WORKSHEET OF CHEMISTRY

STOICHIOMETRY

By: Dasianto, S.Pd

SMA BRAWIJAYA SMART SCHOOL MALANGJl. CIPAYUNG 10 MALANG

STOICHIOMETRY

1. Reaction EquationAt junior high school level, we have studied about material changes. There are chemical and physical

changes. physical changes are usually only indicated by the occurrence of phase transition, for example, from liquid to solid (frozen), from liquid to gas (evaporates) and others. While chemical changes are not limited to changes in the form of substance, but also change the properties, structure and composition of substance. Chemical changes are usually indicated by several changes. The changes are:1. Change of temperature 2. Change of colour3. The formation of gas4. The formation of precipitate5. New odor appears

To understanding about the chemical change, do this experiment!1. Tittle: Chemical Change2. Purpose: understanding characteristic of chemical change3. Materials and equipmnets

Materials Equipments HCl 0,1 M Test tubeMagnesium ribbon Thermometer KI 0,1 M Pippet Pb(NO3)2 0,1 MNa2S 0,1 M

4. Procedure and experiment dataNo Procedure Experiment data 1 First experiment

a. Take 5 mL of HCl 0,1 M and place in test tubeb. Measure the temperature of HCl solutionc. Enter the magnesium ribbon to the test tubed. Observe the changes, and measure the

temperature in test tube

Initial temperature:Final temperature:Another observation:

2 Second experimenta. Take 3 mL of Pb(NO3)2 solution and place in

test tubeb. Add KI solution drop by drop (using pippet)

Initial colour of each substance:Pb(NO3)2:KI:Final colour of mixture:Another observation:

3 Third experimenta. Take 3 mL of Na2S solution and place in test

tubeb. Add HCl solution drop by drop (using pippet)c. Smell the odor of the mixture

Odor that appears:

5. AnalysisNo Questions Answers 1 What is (are) that indicate chemical change

in first, second and third experiment? First experiment:

Second experiment:

Third experiment:

2 Predict product of first, second and third reaction reaction!

6. Conclussion:

The another example of a chemical change is rusty of iron. Iron which was originally shiny and silvery be changed to brown due to chemical changes. To symbolize a chemical change called the reaction equation. Rusty of iron symbolized by:

4Fe(s) + 3O2(g) + 5H2O(l) 2Fe2O3 . 5H2O(s)From the equation above, rusty of iron needed oxygen and water. Fe is symbol of iron, O2 symbol of oxygen, H2O symbol of water, Fe2O3 . 5H2O symbol or rust. While (l), (s), (g) are symbols of physical state of substance. s = solid, l = liquid, g = gas, aq = aqueous. What is the meaning 3 and 2 in 3O2? 3 is coefisient reaction (explain how many molecules that needed in reaction), 2 is index (explain how many atom in a molecule). Arrow () explain direction of reaction from reactant (substances in left side or needed for reaction) to product (substance in right side or product of reaction). Based on information above, write the reaction equation for first and second experiment!

In a reaction equation we know some term. Coefficient, index, physical state etc. Function of coefficient is to make amount of atom in reactant and product are balance. Its process called as balancing reaction equation. Example: make this reaction equation balance: Na(s) + Cl2(g) NaCl(s)Number of sodium atom in left and right is balance, but number of chlorine atom in left and right side unbalance. To make it balance, place number 2 in front of NaCl and Na to become it coefficient. 2Na(s) + Cl2(g) 2NaCl(s)

Excercise: Balance these reactions equation:No Questions Answers 1 Mg(s) + O2(g) MgO(s)

2 CO(g) + O2(g) CO2(g)

3 Al(s) + O2(g) Al2O3(s)

4 CH4(g) + O2(g) CO2(g) + H2O(g)

5 C2H6(g) + O2(g) CO2(g) + H2O(g)

6 C3H6(g) + O2(g) CO2(g) + H2O(g)

7 Ca(s) + HCl(aq) CaCl2(aq) + H2(g)

8 Al(s) + H2SO4(aq) Al2(SO4)3 + H2(g)

9 Mg(NO3)2(aq) + NaCl(aq) MgCl2(aq) + NaNO3(aq)

10 NH4Cl(aq) + Ba(OH)2(aq) NH4OH(aq) + BaCl2(aq)

11 Na2SO4(aq) + Ca(OH)2(aq) CaSO4(s) + NaOH(aq)

12 C2H5OH(aq) + O2(g) CO2(g) + H2O(g)

13 NaOH(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l)

14 CaC2(s) + H2O(l) Ca(OH)2(aq) + C2H2(g)

15 Pb(s) + H2SO4(aq) Pb2(SO4)3(aq) + H2(g)

There are several types of chemical reaction:a. Combination reaction

Combination reaction or additon reactionis that in which a compound is formed from elements or some simpler compounds. Example:2Mg(s) + Cl2(g) 2MgCl(s)PCl3(g) + Cl2(g) PCl5(g)

b. Decomposition reactionDecomposition reaction is one in which a compound breaks down into simpler substances (elements or compound). Example:2H2O(l) 2H2(g) + O2(g)CaCO3(s) CaO(s) + CO2(g)

c. Displacement reactionin a displacement reaction one element displaces another element from a compound; that is one element leaves the compound and another element takes its place. Example:Al(s) + H2SO4(aq) Al2(SO4)3 + H2(g)

d. Double displacement reactiondouble displacement reaction (metethesis reaction) is a reaction in which two compound exchange part (ussualy) ions. Example:Mg(NO3)2(aq) + NaCl(aq) MgCl2(aq) + NaNO3(aq)

e. Combustion reactiona combustion reaction is a reaction of an element or a compound with oxyges gas to produces heats, light or other. Example:CH4(g) + O2(g) CO2(g) + H2O(g)

Excercise: identify types of chemical reaction:No Questions Answers 1 2CO(g) + O2(g) 2CO2(g)

2 2Al(s) + 3Cl2(g) 2AlCl3(s)

3 CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

4 Ca(s) + 2HCl(aq) CaCl2(aq) + H2(g)

5 2NH4Cl(aq) + Ba(OH)2(aq) 2NH4OH(aq) + BaCl2(aq)

6 Na2SO4(aq) + Ca(OH)2(aq) CaSO4(s) + 2NaOH(aq)

7 C(s) + 2H2(g) CH4(g)

8 NH4OH(aq) NH3(g) + H2O(l)

9 2Fe(s) + 6HCl(aq) 2FeCl3(aq) + 3H2(g)

10 2HF(aq) + Ba(OH)2(aq) BaF2(aq) + 2H2O(l)

2. Foundamental Chemical LawThere are five foundamental chemical laws that needed to sudy chemistry. Conservation of mass, definate of proportions, multiple porposition, combining volume and Avogadro’s hypothesis.a. The law of conservation of mass (Lavoisier‘s law)

Total mass reamains constant during a chemical change (chemical reaction) or mass is neither created nor destroyed in chemical reaction. Lavoisier demonstrated that when hydrogen gas (H2) burn and combines with oxygan gas (O2) in a closed container to produces water (H2O), the mass of water obtained is equal to the mass of hydrogen and oxygen gas comsumed.

2H2(g) + O2(g) 2H2O(g)2 grams 1 gram 3 grams

b. The law of definite of proportion (Proust’s law)

Proust said: a given compound always contain exactly the same proportion of element by mass. For example: Proust found that the substance copper(II) carbonate, (CuCO3), is always 5.3 part of copper, 1 part of carbon and 4 part of axygen by mass. How to determine this value?Mass of Cu : mass of C : mass of O1 x atomic mass of Cu : 1 x atomic mass of C : 3 x atomic mass of O1 x 63.55 : 1 x 12.01 : 3 x 15.995.29 : 1 : 4 or 5.3 : 1 : 4

c. The law of multiple proportion (Dalton’s law)Dalton said: when two elements forms a series of compounds, the different masses of one element that combine with the same mass of other element are in the ratio of small whole-number.Example: carbon and oxygen gas if combine able to produce carbon monoxide (CO) and carbon dioxide (CO2) compunds. What is proportion mass of carbon in CO and CO2?

Atoms In CO In CO2

C 1 1O 1 2

To determine proportion mass of carbon atom in CO and CO2, make the oxygen in the same number: Atoms In CO In CO2

C 1 1O 1 2

x2 x1

become:Atoms In CO In CO2

C 2 1O 2 2

So, proportion mass of carbon in CO and CO2 is 2: 1

d. The law of combining valume (Gay Lussac law)Gay Lussac said: the volume of two reacting gas (at the same pressure and temperature) are in the ratio of simpler integers. Moreover, the ratio of the volume of ach product gas to the volume either reacting gas is the ratio of simpler integers. In simple definition, proportion of volume gas in a reaction is equal with proportion of coefficient reaction. Example: N2(g) + 3H2(g) 2NH3(g)Proportion of coeeficient: 1 : 3 : 2Proportion of volume: 1 : 3 : 2If 1 liter of nitrogen gas react with 3 liters of hydrogen gas will produce 2 liters of ammonia (NH3).

e. Avogadro’s hypothesisAvogadro said: equal volumes of different gasses (at the same pressure and temperature) contain equal number of particles. The meaning of particles are ions, atoms or molecules. Number of particles symbolized by mole (n).

or

Example: in container with volume 5 liter places 2 moles of nitrogen gas (N2). In the pressure and temperature, determine volume of oxygen gas (O2) if numbers of its moles is 5!

V2 = 12,5 liters

Exercise: No. Questions Answers1 32 grams of sulfure (S) react with 32 grams of

oxygen (O2) to produce sulfur dioxide (SO2). Predict mass of SO2 that produced!

2 32 grams of sulfure (S) react with 32 grams of

oxygen (O2) to produce sulfur dioxide (SO2). If atomic mass (Ar) sulfure is 32 and oxygen is 16, calculate mass proportion of sulfure and oxygen in sulfur dioxide!

3 Hydrogen (H2) ang oxygen (O2) if combined able to make water (H2O) and hydrogen peroxide (H2O2). Determine mass proportion of oxygen atom in H2O and H2O2!

4 Give attention to the equation reaction:2CO(g) + O2(g) 2CO2(g)If reaction need 40 L of CO, calculate volume oxygen that needed and volume carbon dioxide that produced in this reaction!

5 In a container with volume 2 L, there are 1 mole of methane (CH4) gas. At the same pressure and temperature, calculate volume of propane (C3H8) gas with number of moles are 3!

6 Nitrogen (N2) and oxygen (O2) if combine each other able to make some compounds: NO, N2O, NO2, N2O4 and N2O5. Determine mass proportion nitrogen atom in NO, N2O, NO2, N2O4 and N2O5!

7 Give attention to this data:Mass of H2

Mass of O2

Mass of H2O

Remain

1 8 9 -2 8 9 1 gram of H2

2 18 18 2 grams of O2

3 24 27 -

Determine mass proportion of hydrogen (H) and oxygen (O) atoms in H2O!

8 Give attention to this equation reaction:N2(g) + H2(g) NH3(g) (unbalance)To produce 100 L ammonia, determine volume of nitrogen and hydrogen that needed!

9 In a container with volume 5 L, there are 3 mole of sulfure dioxide (SO2) gas. At the same pressure and temperature, calculate volume of sulfure trioxide (SO3) gas with number of moles are 8!

10 Give attention to this data:Mass of Mg

Mass of O2

Mass of MgO

Remain

3 4 7 -4 4 7 1 gram of Mg3 6 7 2 grams of O2

Calculate mass of megnesium and oxygen that needed to make 56 grams og MgO!

3. Mole ConceptYou have studied that ratio of atoms in a compound are expressed by whole-number subscripts in chemical formula. Fractional numbers are not used because fractions of atoms are not found in compound. For example, in water, H2O, the combining ratio is 2 whole atoms of H to 1 whole atom of O, the subscript ‘1’ is not written. Thus, to make one molecule of H2O, we are bound by th formula of water to take two atom of hydrogen and one atom of oxygen.

2 atoms H + 1 atom H 1 molecule H2OTo make a dozen (12) molecules of H2O, we must take 2 dozen of atom H, and 1 dozen of atom O, still ratio of 2 : 1.

2 dozen atoms H + 1 dozen atoms O 1 dozen molecules H2O.Thus, wheter we express it by atoms or by dozens of atoms, the ratio in H2O is the same, 2H : 1O. This ratio is the stoichiometric law for water. Every pure substance has a stiociometric law disclosed by its formula. Because of the extreme smalless of atoms and molecules, we need far more than dozen of them to have sample we can manipulate. Chemist define a very large standar sample, a quantity called mole. Mole is the international unit for amount of chemical substance. Based on Avogadro experiment, one mole of substance containt 6.02 x 1023 particles. This constanta in the number of formula unit and symbolized by NA.From this constanta we can determine number of particles each substance. example:1 mole of Fe contain 6.02 x 1023

atoms of Fe1 mole of NH3 contain 6.02 x 1023 molecules of NH3

1 mole of NaCl contain 6.02 x 1023 formula units of NaCl

Mole is important concept in chemistry. From mole we can calculate mass of substance, volume of gas and solution, and calculate particles number of substance. Before discuss relation mole and number of substances, we discuss about molecular mass and formula mass firts.a. Molecular mass and formula mass

Molecular mass (Mr) is the sum of atomic mass of all atoms in a molecule, while formula mass (Mr) is the sum of atomic mas formula units of any compound. Uits of (Mr) is amu (atomic mass unit)Example: mass number of C = 12, H = 1. Calculate molecular mass (Mr) of CH4.Molecular mass (Mr) of CH4 = (1 x atomic mass of C) + (4 x atomic mass of H)

= (1 x 12) + (4 x 1)= 16 amu

Exercise: calculate Mr of each substance below:No. Questions Answers No. Questions Answers1 H2O

Water

6 (NH4)2SO4Ammnium sulpfate

2 NH3

Ammonia

7 H2SO4Sulfuric acid

3 PCl3phosphrous

trichloride

8 HNO3Nitric acid

4 SO2

Sulfure dioxide

9 H3PO4Fhosphate acid

5 CO2

Carbon dioxide

10 SF6Sulfure hexasulfide

Atomic mass of H = 1, O = 16, N = 14, S = 32, C = 12, P = 31, F = 19, Cl = 35,5

b. Relation mole and number of substanceRelation mole and number of substance shown by picture below:

Based on the picture above, from mole we can calculate mass of substance, volume of gas, molarity of solution and amount of particles. In other hand, we can calculate mass from volume gas, calculate volume gas from amount of particles etc, by using mole concept.Example:Calculate volume of O2 (at standard temperature and pressure/STP) if mass of oxygen is 3,2 grams and atomic mass of O = 16.

Mr of oxygen = 2 x atomic mass of O= 2 x 16= 16 amu

Moles of oxygen = 0.1 mole Volume of oxygen = mole x Vm

Volume of oxygen = 0.1 mole x 22.4 L/moleVolume of oxygen = 2.24 L

Exercise:No. Questions Answers1 Calculate mole(s) of:

a. 4 grams of NaOHb. 13.2 grams of (NH4)2SO4

c. 3.01 x 1022 molecules of N2

d. 1.204 x 1021 molecules of CH4

e. 1.12 L of H2 gas at STPf. 3.36 L of SO3 gas at 0oC, 1 atmg. 100 mL NaCl 0.1 Mh. 250 mL KOH 0.01 M

Mass number of Na = 23, H = 1, O = 16, N = 14, S = 32, Cl = 23.5

2 Calculate:a. Mass of 6.02 x 1022 SO2 moleculesb. Mass of 5.6 L NH3 gasc. Molarity of 1 gram CaCO3 dissolved into 100

mL of waterd. Molarity of 2.24 L HCl gas dissolved into 500

mL watere. Volume of 9.6 gram SO3 at STP!f. Volume of 3.01 x 1021 molecules NH3

g. Number of molecules of 1.7 gram NH3

h. Number of molecules of 3.36 L NH3 at STP

Mass number of S = 32, O = 16, Ca = 40, C = 12, H = 1, N = 14, Cl = 35.5

4. Chemical CalculationIn this part of the worksheet, we will discuss about chemical calculation. Chemical calculation is calculate substance involve in chemical reaction. How many reactant are consume and how many product that produced are the main of concept in this part. Chemical equation reaction and mole concept are very important thing. Proportion of coefficient reaction equal with proportion number of mole. Example: 1. Given a reaction equation: N2(g) + 3H2(g) 2NH3(g)

Proportion of coefficent reaction: 1 : 3 : 2Proportion of mole: 1 : 3 : 2From the reaction equation above: 1 mole of nitrogen react with 3 moles of hydrogen will produce 2 moles of ammonia.

2. 2.4 gram of magnesium (Mg) react with excess hydrochloric acid (HCl) to produce magnesium chloride and hydrogen gas. Calculate volume of hydrogen in standart temperature and pressure (STP)! (atomic mass (Ar) of Mg = 24.Step to finish the problem:- Calculate mole of Mg

Moles of Mg = 0.1 mole- Balancing equation reaction

Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g)- Calculate mole of H2

Coefficient Mg : H2 = 1 : 1Moles Mg : H2 = 1 : 1 = 0.1 : 0.1

- Calculate volume of H2

Volume H2 = moles x Vm

Volume H2 = 0,1 moles x 22.4 L/moles Volume H2 = 2.24 L

Excercise:No. Questions Answers1 2.7 gram aluminum (Al) react with excess hydrochloric

acid (HCl) to produce aluminum chloride (AlCl3) and hydrogen gas (H2). If Ar of Al = 27, H = 1, Cl = 35,5 determine:a. moles number of Alb. reaction equation

c. mass of AlCl3 that producedd. volume gas that produced at STP

2 Give attention to the reaction equation:CaCO3(s) + 2HCl(aq) CaCl2(aq) + H2O(l) + CO2(g)Calculate mass of CaCO3 that needed to produce 5.6 L gas CO2 at STP! Ar Ca = 40, C = 12, O = 16.

3 Give attention to the reaction equation:CH4(g) + O2(g) CO2(g) + H2O(g) (unbalance)Calculate number of oxygen molecules that needed to burn 3.2 gram methane gas (CH4)! Ar C = 12, H = 1, NA

= 6.02 x 1023.

4 X gram of magnesium (Mg) react with 100 mL HCl 0.1 M

based on the reaction equation:Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g)If Ar Mg = 24, Calculate value of X!

5 Give attention to this reaction:

2Al(s) + 3H2SO4(aq) Al2(SO4)3 + 3H2(g)if x mL H2SO4 0,1 M reacted, produced 2.24 L gas NH3 at STP. Calculate value of x!

6 Give attention to this reaction:

X(s) + 2HNO3(aq) X(NO3)2(aq) + H2(g)If 5.6 gram x reacted produce 2.24 L gas H2 at STP. Calculate Ar of X!

7 Give attention to this reaction equation:NH4Cl(aq) + NaOH(aq) NH3(g) + H2O(l) + NaCl(aq)If 100 mL NH4Cl 0.1 M react completely with NaOH, calculate volume NH3 gas when measured at the same pressure and temperature 2 moles of oxygen has volume 5 L.

8 Give attention to this reaction:Na2SO3(aq) + 2HCl(aq) SO3(g) + H2O(l) + 2NaCl(aq)If 200 mL Na2SO3 0.1 M react completely with HCl, calculate volume SO3 gas when measured at the same pressure and temperature 16 grams of oxygen (Ar = 16) has volume 3 L.

9 Give attention to this reaction:Na2CO3(aq) + 2HCl(aq) CO2(g) + H2O(l) + 2NaCl(aq)If 100 mL Na2CO3 0.2 M react completely with HCl, calculate volume CO2 gas when measured at the same pressure and temperature 3,2 grams of oxygen (Ar = 16) has volume 5 L.

10 Give attention to this reaction:Na2CO3(aq) + 2HCl(aq) CO2(g) + H2O(l) + 2NaCl(aq)If 100 mL Na2CO3 0.2 M react completely with HCl, calculate volume CO2 gas when measured at 27oC and 2 atm, 3.2 grams of oxygen (Ar = 16) has number of volume 5 L.

All of the questions above only one reactant are known. Commonly variable of all reactant are known in a reaction. These condition, make a reaction more complex. Any reactant are completely reacted or in excess number. Example: 32 grams sulfure react with 32 grams oxygen to produce sulfur dioxide. Calculate mass of sulfure dioxide that produced! Ar S = 32, O = 16.

Moles of S = 32/32 = 1 molMoles of O2 = 32/32 = 1 molEquation reaction: S(s) + O2(g) SO2(g)Initial mole : 1 mole 1 moleReacted mole : 0.5 mole 1 mole - 1 mole +Final mole : 0.5 mole - 1 mole

Sulfure has reamain in final reaction called as remain reactan, but O2 completely reacted. O2 called as limitting reactant. SO2 that produced is 1 mole. Mass of SO2 = mole x Mr = 1 mole x 64 g/mole = 64 gramSo the reaction produce 64 grams of SO2. Excercise:

No. Questions Answers1 32 gram of SO2 gas react with 32 grams of oxygen to

produce SO3 based on this equation reaction:2SO2(g) + O2(g) 2SO3(g)If Ar S = 32, O = 16, determinea. Excess reactantb. Mass of excess reactantc. Limitting reactant d. Mass of SO3 that produced!

2 Give attention to this equation reaction:Mg(s) + Cl2(g) MgCl2(s)2.4 grams of magnesium react with 3.55 gram of chlorine. If Ar of Mg = 24, Cl = 35.5 determine:a. Excess reactantb. Mass of excess reactantc. Limitting reactant d. Mass of MgCl2 that produced!

3 Give attention to this equation reaction:2Al(s) + 6HCl(aq) 2AlCl3(aq) + 3H2(g)5.4 grams of aluminum react with 3.65 grams of hydrochloric acid. If Ar Al = 27, H = 1, Cl = 35.5, determine:a. Excess reactantb. Mass of excess reactantc. Limitting reactant d. Mass of AlCl3 that produced!e. Volume hydrogen gas at 0oC, 1 atm.

4 Give attention to this equation reaction:2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g)2.7 grams of aluminum react with 100 mL sulfuric acid 0.1 M. If Ar Al = 27, S = 32, O = 16, H = 1, determine:a. Excess reactantb. Limitting reactant c. Mass of Al2(SO4)3 that produced!d. Volume hydrogen gas at 0oC, 1 atm.

5 Give attention to this equation:Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)100 mL lead(II) nitrat 0.2 M react with 100 mL potassium iodide 0.2 M. Determine:a. Excess reactantb. Limitting reactant c. Mass of PbI2 that produced

6 Give attention to this equation reaction:NH4Cl(aq) + KOH(aq) NH3(g) + H2O(l) + KCl(aq)100 mL ammonium chloride 0.2 M react with 50 mL potassium hydroxide 0.2 M. Determine:a. Excess reactantb. Limitting reactant c. Volume ammonia gas at STP that produced

7 Give attention to this equation reaction:

X(s) + 2HNO3(aq) X(NO3)2(aq) + H2(g)If 2.7 grams of X react with 100 mL HNO3 1M produce 2.24 L hydrogen gas, determine Ar of X!

3. Concentration Unitsa. Mass percentb. Volume percentc. Part per million

4. Molecular Formula, Empirical Formula and Hydrate Compoundsa. Molecular formula and empirical formulab. Hydrate compounds

5. Evaluation1. Pada reaksi

pembuatan gas amonia, persamaan reaksinya adalah:

N2 (g) + 3H2 (g) → 2NH3 (g)Pernyataan yang benar tentang persamaan reaksi di atas adalah....a. Gas amonia disebut zat pereaksib. Angka 3 dalam gas hidrogen dinamakan

indeks reaksic. Gas nitrogen dan gas hidrogen disebut zat

hasil reaksi d. 2 molekul gas amonia adalah zat hasil reaksi e. Ketiga fase dalam hasil raksi di atas sama ,

yaitu fase cair

2. Penulisan persamaan reaksi yang paling tepat bila padatan kalsium bereaksi dengan gas oksigen menghasilkan padatan kalsium oksida adalah....a. 4K (s) + O2 (g) 2K2O (s)b. 2K (s) + O2 (g) 2K2O (s)c. 2Ca (s) + O2 (g) 2CaO (s)d. Ca (s) + O2 (g) CaO (s)e. Ca (s) + O2 (g) CaO2 (s)

3. Pada reaksi pembakaran :

a C3H8(g) + bO2(g) cCO2(g) + H2O(g) Nilai a,b,c, dan d berturut-turut adalah....

a. 1,5,3,4 c. 1,3,4,5 e. 1,4,3,5b. 5,4,3,1 d. 4,3,5,1

4. Diantara persamaan reaksi berikut yang sudah setara adalah ....a. Cr2O3 + 2Al Al2O3 + Cr

b. Al + H2SO4 Al2SO4 + 3H2

c. C2H5OH + O2 2CO2 + 3H2Od. Mg(OH)2 + 2HCl MgCl2 + 2H2Oe. Cu + H2SO4 CuSO4 + 3H2O + SO2

5. Sebanyak 6,02 x 1022 partikel NaOH (Mr = 40) akan memiliki massa sebesar…a. 2 g c. 20 g e. 40 gb. 4 g d. 25 g

6. Untuk mendapatkan gas Cl2 dapat dilakukan dengan reaksi:

KClO3 + HCl KCl + H2O + Cl2 (belum setara)Agar diperoleh 142 gram gas klorin, maka kalium klorat yang dibutuhkan sebanyak…gram. Ar K = 39, O = 16, H = 1, Cl = 35,5.a. 122,5 c. 61,3 e. 24,5b. 81,7 d. 40,8

7. Gas ammonia, NH3, dapat dihasilkan dari reaksi:

(NH4)2SO4 + 2KOH K2SO4 + 2NH3 + 2H2OVolume gas ammonia yang dihasilkan apabila sebanyak 0,56 liter (NH4)2SO4 digunakan pada reaksi tersebut adalah…a. 1,12 L c. 11,2 L e. 2,24 Lb. 1,20 L d. 22,4 L

8. Cuplikan serbuk besi sebanyak 5 gram dipanaskan dengan gas klorin berlebih dan menghasilkan 10 gram besi(II) klorida. Kadar unsure besi tersebut adalah…(Ar Fe = 56, Cl = 35,5)a. 4,41 % c. 71,0 % e. 100 %b. 14,2 % d. 88,2 %

9. Gas ammonia dapat dihasilkan melalui persamaan reaksi berikut:

(NH4)2SO4(aq) + 2KOH(aq) 2NH3(g) + 2H2O(l) + K2SO4(aq)

Reaksi berlangsung pada 0OC, 1 atm. Volume gas ammonia (NH3) yang dihasilkan setelah 33 gram (NH4)2SO4 (Mr = 132) bereaksi adalah…a. 2,8 liter c. 12,0 liter e. 11,2 literb. 5,6 liter d. 22,4 liter

10. Logam Al sebanyak 0,2 mol dilarutkan ke dalam 600 mL asam sulfat 0,5 M. Volume gas yang terbentuk pada 0oC, 1 atm adalah…L.a. 2,24 c. 4,48 e. 11,2b. 2,90 d. 6,72

11. Sebanyak 40 mL gas P2 tepat bereaksi dengan 100 mL gas Q2 untuk menghasilkan 40 mL gas PxQy pada suhu dan tekanan yang sama. Maka harga x dan y adalah…

a. 1 dan 2 c. 1 dan 5 e. 2 dan 5b. 1 dan 3 d. 2 dan 3

12. Gas X sebanyak 0,2 gram menenpati volume 440 mL. Jika 0,1 gram gas CO2 pada P dan T yang sama, menempati volume 320 mL. Gas X adalah…(Ar C = 12, N = 14, O = 16, S = 32)

a. O2 c. SO3 e. NOb. SO2 d. NO2

13. Suatu senyawa organic berbentuk gas sebanyak 5,6 gram pada keadaan standar mempunyai volume 1,5 L. Jika senyawa tersebut memiliki 86% karbon dan 14% hydrogen, rumus molekul senyawa tersebut adalah…Ar C = 12, H = 1.

a. C2H4 c. C4H8 e. C6H12

b. C3H6 d. C5H10

14. Belerang dapat dihasilkan melalui oksidasi gas H2S, menurut: H2S + O2 S + H2O. Banyaknya belerang yang dapat diperoleh saat mengoksidasi 22,4 L gas H2S (STP) adalah…Ar S = 32

a. 10 g c. 160 g e. 320 gb. 32 g d. 224 g

15. Suatu senyawa mengandung 32,4% natrium, 22,5% belerang dan sisanya oksigen. Jika Ar Na = 23, S = 32 dan O = 32, senyawa tersebut adalah…

a. Na2SO3 c. Na2S2O3 e. Na2S2O7

b. Na2SO4 d. Na2S4O6

16. Reduksi besi(III) oksida dengan CO:

Fe2O3 + CO Fe + CO2 (belum setara)Untuk menghasilkan 11,2 kg besi (Ar Fe = 56) dibutuhkan besi(III) oksida sebesar….Ar O = 16

a. 22 kg c. 18 kg e. 15 kgb. 20 kg d. 16 kg

17. Logam seng yang massanya 6,5 gram direaksikan dengan asam klorida menurut persamaan reaksi :

Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g)Volume gas hidrogen yang dihasilkan pada keadaan standar adalah …. (Ar Zn = 65)a. 2,24 liter c. 4,48 liter e. 5,60

literb. 11,20 liter d. 22,40 liter

18. Dalam 15,9 gram senyawa tembaga(I) sulfide (Ar Cu = 63,5 ; S = 32) terdapat Cu sebanyak ..g.

a. 6,35 c. 15,9 e. 31,8b. 12,7 d. 25,4

19. Pada pembakaran sempurna 5 liter gas asetilena (C2H2) menghasilkan gas karbon dioksida dan uap air menurut persaman reaksi:C2H2(g) + O2(g) CO2(g) + H2O(g) belum setaraPerbandingan zat hasil reaksi pada proses pembakaran tersebut adalah…a. 1 : 2 c. 2 : 5 e. 5 : 2b. 2 : 1 d. 4 : 5

20. Pada percobaan reaksi antara tembaga dan belerang sehingga membentuk.Tembaga (II) sulfida dan data yang diperoleh sebagai berikut.

percobaan

Massatembaga

(g)

Massabelerang

(g)

Massa tembaga sulfida (g)

1234

182888

2345

69

1212

Berdasarkan data tersebut , perbandingan massa tembaga dan belerang sehingga membentuk senyawa tembaga (II) sulfida adalah....a. 1 : 1 c. 1 : 2 e. 2 : 1b. 3 : 1 d. 2 : 3

21. Data percobaan pembakaran belerang:No Massa S Massa O2 Massa SO3

1 0,64 gram 1,92 gram 1,60 gram2 0,32 gram 0,48 gram 0,80 gram3 0,64 gram 0,96 gram 1,60 gram4 0,48 gram 0,96 gram 1,20 gram

Perbandingan massa belerang dan oksigen adalah…a. 1 : 3 c. 2 : 1 e. 3 : 2b. 1 : 2 d. 2 : 3

22. Pada suatu bejana direaksikan 100 mL kalium iodide 0,1 M dengan 100 mL timbal(II) nitrat 0,1 M menurut persamaan reaksi berikut:2KI(aq) + Pb(NO3)2(aq) → PbI2(aq) + 2KNO3(aq)Jika Ar K = 39, I = 127, Pb = 207, N = 14, O = 16, maka pernyataan yang benar adalah…a. Pb(NO3)2 merupakan pereaksi pembatasb. KI merupakan pereaksi pembatasc. KI dan Pb(NO3)2 habis bereaksi

d. Bersisa 0,65 gram Pb(NO3)2

e. Bersisa 1,65 gram KI

23. Given reaction :3Ca(NO3)2(aq) +2Na3PO4(aq) Ca3(PO4)2(s) + 6NaNO3(aq)If10 mL Ca3(PO4)2 1 M mixed 10 mL Na3PO4 2 M, precipitate that produced are… (O = 16; Na = 23; P = 31; Ca = 40)a. 0.85 gram c. 3.10 gram e. 1.55

gramb. 1.03 gram d. 3.95 gram

24. One mole of calcium cyanide (CaCN2) react completely with one mole of water :CaCN2 + H2O CaCO3 + NH3 (unbalanced)Volume of ammonia gas that produced at STP is…a. 67.2 L c. 22.4 L e. 5 Lb. 33.6 L d. 15 L

25. Given reaction :

Fe2(SO4)3(aq) + NaOH(aq) Fe(OH)3(s) + Na2SO4(aq) (unbalanced)If initial mole each reactant is one mole, how many mole of iron(III) hydroxide that produced ?a. 1/3 mole c. 1 mole e. 2/3 moleb. ½ mole d. 3 moles

26. If 0.56 grams of M (a metal) react with HCl to produce 0.005 moles of H2 and MCl2 salt. Atomic relative mass of M is…

a. 7 c. 28 e. 112b. 14 d. 56

27. Aluminum able to react with concentrated KOH based on this reaction : 2Al(s) + 2KOH(l) + 6H2O(l) 2K[Al(OH)4](aq) + 3H2(g)If 2.7 gram Al (Ar = 27) reacted, volume hydrogen gas at STP is…

a. 1.12 L c. 3.36 L e. 5.60 Lb. 2.24 L d. 4.48 L

28. Given reaction :

FeS2(s) + O2(g) Fe2O3(s) + SO2(g) (unbalanced)How many gram(s) of FeS2 (Mr 120, purity = 90%) that needed to produce 2.24 L of SO2 at 0oC and 1 atm ?a. 5.4 g c. 6.7 g e. 21.6 gb. 6.0 g d. 12.0 g

29. 3 grams of aluminum dipped into copper(II) sulphate solution :

Al(s + 3CuSO4(aq) Al2(SO4)3 + Cu(s)Copper that produced used to produce NO2 gas :

Cu(s) HNO3(aq) Cu(NO3)2(aq) + NO2(g) + H2O(l) (the reactions unbalanced). Volume SO2 (STP) that produced is….a. 1.3 L c. 3.4 L e. 8.5 Lb. 1.7 L d. 7.4 L

30. Given reaction :

KClO3(aq) + 6HCl(aq) KCl(aq) + 3H2O(l) + 3Cl2(g)To produce 213 grams of chlorin gas, need potassium chlorate…. grams. Ar H = 1, O = 16, K = 39, Cl = 35.5)a. 40.8 c. 122.5 e. 367.5b. 61.25 d. 183.75

31. 5.8 grams of a bivalence base [M(OH)2] react completelly with 200 mL HCl 1 M :

M(OH )2(s) +HCl (aq) → MCl2(aq) + H2O(l) (unbalanced)

Relative atomic mass of M is… (Ar H=1, O=16 )a. 24 c. 28 e. 58b. 27 d. 40

32. 21.75 grams of pyrolusite (MnO2) react with hydrochloric acid : MnO2(s) + 2HCl(aq) MnCl2(aq) + H2O(l) + Cl2(g)

If in the same temperature and pressure, mass of one liter NH3 is 8.5 gram, so volume of chlorin gas is… (Ar Mn = 55, O = 16, N = 14, H = 1, Cl = 35.5)a. 125 mL c. 500 mL e. 1000 mLb. 250 mL d. 750 mL

33. 32.5 grams of iron(III) chloride react with sodium carbonate :

2FeCl3(aq) + 3Na2CO3(aq) + 3H2O(l) 2Fe(OH)3(s) + 6NaCl(aq) + 3CO2(g)Which statement is not true ?a. Precipate that produce are 21.4 gramsb. Gas that produce are 6.72 L (STP)c. Gas that produce are 10 L (27oC, 2 atm)d. Sodium carbonate that needed are 31.8 gramse. Sodium chloride that produce are 35.1 grams

34. 8 grams of sulphure react with 16 grams of oxygen to produces sulphure threeoxide gas. Which statement is not true ?

a. Sulphure as limiting reagentb. Remain of oxygen is 4 gramsc. Sulphure threeoxide gas that produces is 20 gramsd. Proportion of oxygen and sulphure is 4 : 5e. To produce maximum sulphure threeoxide gas,

all of sulphure must be react

35. For the reaction : Mg(s) + CuSO4(aq) MgSO4(aq) + Cu(s)

Proportion mass of Mg and Cu is…a. 2 : 1 c. Mg > Cu e. Mg = Cub. 3 : 3 d. Mg < Cu