28 Sep How many moles of C are produced from 1 mol of A?

CHEM1305 Introductory Chemistry

Chapter 9 Homework Assignment  

Question 1Consider the general chemical equation:  A  +  2 B  →  3 C

How many moles of C are produced from 1 mol of A?

 

  1

 

  2

 

  3

 

  4

 

 Question 2Given the decomposition of hydrogen peroxide, calculate the moles of oxygen gas produced from 5.00 mol of H2O2

 

2 H2O2(l)  →  2 H2O(l)  +  O2(g)

 

  1 mol

 

  2.5 mol

 

  5 mol

 

  10 mol

 

 Question 3How many moles of propane gas, C3H8, react with 1.29 mol of oxygen gas?

 

C3H8(g)  +  5 O2(g)  →  3 CO2(g)  +  4 H2O(g)

 

  6.45 mol

 

  0.258 mol

 

  1 mol

 

  5 mol

 

 Question 4Given the balanced equation, calculate the mass of H2 that can be prepared from 141 g Al.

 

2 Al(s)  +  6 HNO3(aq)  →  2 Al(NO3)3(aq)  +  3 H2(g)

 

  212 g

 

  1.50 g

 

  5.22 g

 

  15.8 g

 

 Question 5Given the balanced equation, calculate the mass of Cl2 required to produce 6.78 g of PCl3.

 

2 P(s)  +  3 Cl2(g)  → 2 PCl3(l)

 

  5.25 g

 

  137 g

 

  10.2 g

 

  70.9 g

 

 Question 6What mass of CO2 will react with 1.00 g LiOH?

 

2 LiOH(s)  +  CO2(g)  →  Li2CO3(s)  +  H2O(l)

 

  1.84 g

 

  0.500 g

 

  2.00 g

 

  0.920 g

 

 Question 7If 9.00 moles of hydrogen gas and 9.00 moles of oxygen gas are combined, what is the limiting reactant?

 

2 H2(g)   +   O2(g)  →   2 H2O(l)

 

  H2

 

  O2

 

  H2O

 

 Question 8If 50.0 g of Co react with 30.0 g of S, which compound is the limiting reactant?

 

Co(s)   +   S(s)  →   CoS(s)

 

  Co

 

  S

 

  CoS

 

 Question 9A manufacturer performs a chemical reaction to produce sulfur hexafluoride, SF6. After the reaction is complete, 480.2 kg is isolated. If the theoretical yield of SF6 was 546.7 kg, what was the percent yield of the reaction?

 

  113.8%

 

  87.84%

 

  26.25%

 

  48.02%

 

 Question 10A student dissolves 1.50 g of copper(II) nitrate in water. After adding aqueous sodium carbonate solution, the student obtains 0.875 g of CuCO3 First, calculate the theoretical yield of the CuCO3 and next use that to calculate the percent yield for this student’s experiment. What is the percent yield?

 

Cu(NO3)2(aq)   +   Na2CO3(aq)  →   CuCO3(s)   +   2 NaNO3(aq)

 

  58.3%

 

  88.6%

 

  113%

 

  100%