Chemistry 2202

Unit 1 Part 2 ICA

Name:_______________

Part 1: Write the letter of the correct response to each question in the space provided: 1.____

5.____

9.____

13.____

17.____

2.____

6.____

10.____

14.____

18.____

3.____

7.____

11.____

15.____

4.____

8.____

12.____

16.____

1.

What mass of chlorine gas, Cl2, is required to react with exactly 5.00 g of iron to produce 14.5 g of iron(III) chloride, FeCl3? 2 Fe(s)



3 Cl2(g)

5.00 g

A. B. C. D. 2.

14.5 g

5.00 g 7.50 g 9.50 g 21.8 g

According to the balanced equation below, what mass of magnesium is expected to react with one mole of fluorine gas? A. B. C. D.



F2(g)



MgF2(s)

1.00 g 24.31 g 38.00 g 62.31 g

Which mole ratio should be used to calculate the number of moles of carbon dioxide gas produced from the combustion of 0.45 moles of C4H10? 2 C4H10(g)

4.

2 FeCl3(s)

?

Mg(s)

3.





13 O2(g)



8 CO2(g)



10 H2O(g)

A.

 2 mol O2     8 mol CO2 

C.

 8 mol CO2     2 mol C4H10 

B.

 2 mol C4H10     8 mol CO2 

D.

 8 mol C4H10     2 mol CO2 

How many moles of oxygen gas are required to completely burn 1.54 mol of ethane? 2 C2H6(g)

A. B. C. D.



7 O2(g)

0.0548 mol 0.440 mol 5.39 mol 10.8 mol



4 CO2(g)



6 H2O(g)

5.

What is used in gravimetric stoichiometry? A. mass B. volume C. molecules D. formula units

6.

What mass of magnesium nitride (molar mass = 100.95 g/mol) should be produced when 0.810 mol magnesium reacts? 3 Mg(s)

A. B. C. D. 7.



N2(g)



Mg3N2(s)

3.33 g 8.18 g 19.6 g 27.3 g

What are the products of the complete combustion of a hydrocarbon? A. C(s) & H2(g) B. CO(g) & H2O(g) C. CO2(g) & H2O(g) D. CO(g) & H2O(l) The unbalanced equation below shows the reaction between aqueous solutions of nickel (II) sulfate and barium chloride. Use this equation for #8 & #9 __ Ni2(SO4)3 + __ BaCl2  __ BaSO4 + __ NiCl3

8.

In order (from left to right), what are the correct coefficients for the balanced equation? A. 1, 2, 3, 2 B. 0, 3, 3, 2 C. 1, 3, 3, 2 D. 2, 4, 3, 2

9.

Which of the four chemicals in the reaction will have the subscript (s) A. Ni2(SO4)3 B. BaCl2 C. BaSO4 D. NiCl3

10.

Silicon can be produced by reacting silicon tetrachloride with pure magnesium. Based on the given amounts below, which species is correctly identified? SiCl4(g)



0.45 mol

A. B. C. D.

SiCl4 Mg Si MgCl2

limiting species limiting species excess species excess species

2 Mg(s) 0.80 mol



Si(s)



2 MgCl2(s)

11.

How many moles of silicon should be produced based on the given amounts? SiCl4(g)



0.45 mol

A. B. C. D. 12.

2 Mg(s)



0.80 mol

Si(s)



2 MgCl2(s)

? mol

0.40 mol 0.45 mol 0.80 mol 1.25 mol

A science fair project showed the neutralization of excess stomach acid (HCl) by an antacid, sodium hydrogen carbonate, NaHCO3. The reaction produced carbon dioxide gas bubbles. HCl(aq)



NaHCO3(aq)



NaCl(aq)



H2O(l)



CO2(g)

When the reaction was complete, the student added a few more drops of hydrochloric acid (stomach acid) to the beaker and noticed that no additional bubbles formed. Which interpretation of the observations is correct? A. B. C. D.

the excess species is carbon dioxide the excess species is sodium chloride the limiting species is hydrochloric acid the limiting species is sodium hydrogen carbonate

13.

What are the formulas for the products of the reaction between AgNO3 and Cu? A. CuAg2 & NO3 B. Cu(NO3)2 & Ag C. Cu + N2 + Ag + O2 D. CuO + Ag3N

14.

Sheldon and Leonard worked together to complete a gas stoichiometry lab activity. Their calculations indicated that the reaction should produce 27.9 mL of CO2 gas at room temperature. After working very carefully, they collected 21.6 mL of CO2. How should they classify the 27.9 mL volume of product? A. actual yield B. percent yield C. random yield D. theoretical yield

15.

Sara and Andrew worked carefully to complete a gravimetric stoichiometry activity in which they collected 2.45 g of silver chloride precipitate. Their calculations indicated that this reaction should produce 3.89 g of product. What was their percent yield? A. 37.0 % B. 63.0 % C. 100 % D. 158 %

16.

Which substance has low solubility in water? A. AgCH3COO B. Fe(NO3)3 C. BaBr2 D. (NH4)2SO4

17.

Which term means ‘the chemical that is completely used in a chemical reaction’ ? A. B. C. D.

18.

excess species gravimetric species limiting species product species

Which is determined by stoichiometric calculations? A. actual yield B. random error C. systematic error D. theoretical yield

Part 2 – Constructed Responses: Write your responses in the spaces provided. workings. Follow the significant digits/rounding rules.

Show all

19. Iron ore reacts with carbon monoxide in a blast furnace to produce molten iron. In a test reaction, 120 g of iron(III) oxide is reacted with excess carbon monoxide. Calculate the mass of carbon dioxide (at STP) that should be produced. (4) Fe2O3(s) +

CO(g) →

Fe(s) +

CO2(g)

20. Write the balanced equation with subscripts for the reaction between: a)

aqueous solutions of lead(II) nitrate and sodium sulphide

b)

aluminum and chlorine

21.

Use the equation provided to determine: K

+

S8 →

K2S

a) the number of moles of sulfur needed to react with 75.4 g of potassium. (3)

b) the mass of potassium sulfide that will be produced if 0.500 mol of sulfur reacts. (2)

22.

Calculate the volume of hydrogen gas at STP that should be produced by the decomposition of 3.56 g of water. (4) H2O →

H2 +

O2

22. A 2.00 g pellet of a sodium hydroxide is placed in a beaker containing 0.0600 mol of sulfuric acid, (H2SO4(aq) ). Determine the limiting species in this reaction. (2) 2 NaOH(s) +

H2SO4(aq) → Na2SO4(aq) + 2 H2O(l)

23. Dave and Morley reacted 3.00 g of Cu with excess silver nitrate. They isolated the silver product by filtration. 2 AgNO3 (aq)



Cu(s)



Cu(NO3 )2(aq)



2 Ag (s)

a)

Calculate the theoretical yield of silver. (3)

b)

Dave and Morley recorded an actual yield of 11.50 g of Ag. Calculate the percent yield. (1)

Chemistry 2202

Unit 1 Part 2 ICA

Name:_______________

Part 1: Write the letter of the correct response to each question in the space provided: 1.____

5.____

9.____

13.____

17.____

2.____

6.____

10.____

14.____

18.____

3.____

7.____

11.____

15.____

4.____

8.____

12.____

16.____

1.

What mass of chlorine gas, Cl2, is required to react with exactly 5.00 g of iron to produce 14.5 g of iron(III) chloride, FeCl3? 2 Fe(s)



3 Cl2(g)

5.00 g

 

2.

A. B. C. D.

3.

14.5 g

5.00 g 7.50 g 9.50 g 21.8 g

According to the balanced equation below, what mass of magnesium is expected to react with one mole of fluorine gas? A. B. C. D.



F2(g)



MgF2(s)

1.00 g 24.31 g 38.00 g 62.31 g

Which mole ratio should be used to calculate the number of moles of carbon dioxide gas produced from the combustion of 0.45 moles of C4H10? 2 C4H10(g)

4.

2 FeCl3(s)

?

Mg(s)







13 O2(g)



8 CO2(g)



10 H2O(g)

A.

 2 mol O2     8 mol CO2 

 C.

 8 mol CO2     2 mol C4H10 

B.

 2 mol C4H10     8 mol CO2 

D.

 8 mol C4H10     2 mol CO2 

How many moles of oxygen gas are required to completely burn 1.54 mol of ethane? 2 C2H6(g)

A. B.  C. D.



7 O2(g)

0.0548 mol 0.440 mol 5.39 mol 10.8 mol



4 CO2(g)



6 H2O(g)

5. 

What is used in gravimetric stoichiometry? A. mass B. volume C. molecules D. formula units

6.

What mass of magnesium nitride (molar mass = 100.95 g/mol) should be produced when 0.810 mol magnesium reacts? 3 Mg(s)

A. B. C.  D.



N2(g)



Mg3N2(s)

3.33 g 8.18 g 19.6 g 27.3 g

7.

What are the products of the complete combustion of a hydrocarbon? A. C(s) & H2(g) B. CO(g) & H2O(g)  C. CO2(g) & H2O(g) D. CO(g) & H2O(l) The unbalanced equation below shows the reaction between aqueous solutions of nickel (II) sulfate and barium chloride. Use this equation for #8 & #9 __ Ni2(SO4)3 + __ BaCl2  __ BaSO4 + __ NiCl3

8.



9.



10.

In order (from left to right), what are the correct coefficients for the balanced equation? A. 1, 2, 3, 2 B. 0, 3, 3, 2 C. 1, 3, 3, 2 D. 2, 4, 3, 2 Which of the four chemicals in the reaction will have the subscript (s) A. Ni2(SO4)3 B. BaCl2 C. BaSO4 D. NiCl3 Silicon can be produced by reacting silicon tetrachloride with pure magnesium. Based on the given amounts below, which species is correctly identified? SiCl4(g)



0.45 mol



A. B. C. D.

SiCl4 Mg Si MgCl2

limiting species limiting species excess species excess species

2 Mg(s) 0.80 mol



Si(s)



2 MgCl2(s)

11.

How many moles of silicon should be produced based on the given amounts? SiCl4(g)



0.45 mol

2 Mg(s)



0.80 mol

Si(s)



2 MgCl2(s)

? mol



A. B. C. D.

12.

A science fair project showed the neutralization of excess stomach acid (HCl) by an antacid, sodium hydrogen carbonate, NaHCO3. The reaction produced carbon dioxide gas bubbles.

0.40 mol 0.45 mol 0.80 mol 1.25 mol

HCl(aq)



NaHCO3(aq)



NaCl(aq)



H2O(l)



CO2(g)

When the reaction was complete, the student added a few more drops of hydrochloric acid (stomach acid) to the beaker and noticed that no additional bubbles formed. Which interpretation of the observations is correct?

 13. 

14.

 15.



16. 

A. B. C. D.

the excess species is carbon dioxide the excess species is sodium chloride the limiting species is hydrochloric acid the limiting species is sodium hydrogen carbonate

What are the formulas for the products of the reaction between AgNO3 and Cu? A. CuAg2 & NO3 B. Cu(NO3)2 & Ag C. Cu + N2 + Ag + O2 D. CuO + Ag3N Sheldon and Leonard worked together to complete a gas stoichiometry lab activity. Their calculations indicated that the reaction should produce 27.9 mL of CO2 gas at room temperature. After working very carefully, they collected 21.6 mL of CO2. How should they classify the 27.9 mL volume of product? A. actual yield B. percent yield C. random yield D. theoretical yield Sara and Andrew worked carefully to complete a gravimetric stoichiometry activity in which they collected 2.45 g of silver chloride precipitate. Their calculations indicated that this reaction should produce 3.89 g of product. What was their percent yield? A. 37.0 % B. 63.0 % C. 100 % D. 158 % Which substance has low solubility in water? A. AgCH3COO B. Fe(NO3)3 C. BaBr2 D. (NH4)2SO4

17.

Which term means ‘the chemical that is completely used in a chemical reaction’ ?



A. B. C. D.

18.



excess species gravimetric species limiting species product species

Which is determined by stoichiometric calculations? A. actual yield B. random error C. systematic error D. theoretical yield

Part 2 – Constructed Responses: Write your responses in the spaces provided. workings. Follow the significant digits/rounding rules.

Show all

19. Iron ore reacts with carbon monoxide in a blast furnace to produce molten iron. In a test reaction, 120 g of iron(III) oxide is reacted with excess carbon monoxide. Calculate the mass of carbon dioxide (at STP) that should be produced. (4) Balance 1st

1 Fe2O3(s) +

Calculate ngiven

n=

Mole Ratio

nCO2 = 0.7514 mol Fe2O3 x

Calculate m

m = 2.254 mol x 44.01 g/mol = 99 g

3 CO(g) →

2 Fe(s) +

3 CO2(g)

= 0.7514 mol Fe2O3 = 2.254 mol CO2

20. Write the balanced equation with subscripts for the reaction between: a)

aqueous solutions of lead(II) nitrate and sodium sulphide Pb(NO3)2(aq) + Na2S → PbS(s) + 2 NaNO3(aq)

b)

aluminium and chlorine 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s)

21.

Use the equation provided to determine: 16 K

+ 1 S8 → 8 K2S

a) the number of moles of sulfur needed to react with 75.4 g of potassium. (3) Calculate ngiven

n=

= 1.928 mol K

Mole Ratio

nS8 = 1.928 mol K x

= 0.2410 mol S8

b) the mass of potassium sulfide that will be produced if 0.500 mol of when sulfur reacts? (2) Mole Ratio

nCO2 = 0.500 mol S8 x

= 4.00 mol K2S

Calculate m

m = 4.00 mol x 110.27 g/mol = 441 g

22.

Calculate the volume of hydrogen gas at STP that should be produced by the decomposition of 3.56 g of water. (4)

2 H2O → 2 H2 + 1 O2 Calculate ngiven

n=

= 0.1976 mol H2O

Mole Ratio

nCO2 = 0.1976 mol H2O x

Calculate m

v = 0.1976 mol x 22.4 L/mol = 4.43 L

= 0.1976 mol H2

23. A 2.00 g pellet of a sodium hydroxide is placed in a beaker containing 0.0600 mol of sulfuric acid, (H2SO4(aq) ). Determine the limiting species in this reaction. (2) 2 NaOH(s) +

H2SO4(aq) → Na2SO4(aq) + 2 H2O(l)

2.00 g

0.0600 mol

Calculate the # of mol of Na2SO4 (or H2O) from each reactant. The limiting reactant produces less product. Using NaOH: Calculate ngiven

n=

= 0.0500 mol NaOH

Mole Ratio

nH2O = 0.0500 mol NaOH x

= 0.0500 mol H2O

nH2O = 0.0600 mol H2SO4 x

= 0.120 mol H2O

Using H2SO4: Mole Ratio

The LR is NaOH because it produces less water. 24. Dave and Morley reacted 3.00 g of Cu with excess silver nitrate. They isolated the silver product by filtration. 2 AgNO3 (aq)

a)



Cu(s)



Cu(NO3 )2(aq)

2 Ag (s)

Calculate the theoretical yield of silver. (3)

Calculate ngiven

n=

Mole Ratio

nAg = 0.04721 mol Cu x

Calculate m

m = 0.09441 mol x 107.87 g/mol = 10.2 g

b)



= 0.04721 mol Cu = 0.09441 mol Ag

Dave and Morley recorded an actual yield of 11.50 g of Ag. Calculate the percent yield. (1)

% yield =

x 100 = 113 %

Product mass is too high – probably not dry!!