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Chapter 16: Energy and Chemical Change

Practice Test
      
  1.Chemical reactions and physical changes that absorb energy from their surroundings are __________.  
  a.   mesothermic  
  b.   endothermic  
  c.   exothermic  
  d.   isothermic  
  Hint    
      
  2.What is the final temperature of a mixture of chromium metal and water when 50.0 grams of chromium at 15°C (specific heat = 0.448 J/(g•°C)) is added to 25 mL of water (specific heat = 4.18 J/(g•°C)) at 45°C? The density of water is 1 g/mL.  
  a.   35°C  
  b.   40°C  
  c.   25°C  
  d.   30°C  
  Hint    
      
  3.Which of the following processes occurs with a decrease in entropy?  
  a.   dissolving salt in water  
  b.   boiling water  
  c.   freezing of water  
  d.   sublimation of dry ice  
  Hint    
      
  4.Calculate the free energy for the following reaction at 25°C.
2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2 (g)
ΔH° (kJ/mol) -205.6 0 -348.3 -296.8
ΔS° v(J/mol•K) 57.5 205.0 43.64 248.1
 
  a.   -951.1 kJ  
  b.   -704.2 kJ  
  c.   -835 kJ  
  d.   -922.6 kJ  
  Hint    
      
  5.How much heat energy is liberated when 11.0 grams of manganese is used in the formation of Mn2O3?
ΔHf° for Mn2O3 is -962.3 kJ/mol
 
  a.   460 kJ  
  b.   289 kJ  
  c.   192 kJ  
  d.   96.3 kJ  
  Hint    
      
  6.If 5.0 grams of copper cools from 35.0°C to 22.6°C and loses 23.6 joules of heat, what is the specific heat of copper?  
  a.   0.38 J/(g•°C)  
  b.   0.62 J/(g•°C)  
  c.   3.8 × 102 J/(g•°C)  
  d.   0.076 J/(g•°C)  
  Hint    
      
  7.The same amount of heat is added to a 10-g sample of each of the following metals. If each metal is initially at 20.0°C, which metal will reach the highest temperature?  
  a.   beryllium 1.82 J/(g•°C)  
  b.   gold 0.129 J/(g•°C)  
  c.   calcium 0.653 J/(g•°C)  
  d.   copper 0.385 J/(g•°C)  
  Hint    
      
  8.How much heat is absorbed in the complete reaction of 3.00 grams of SiO2 with excess carbon in the reaction below?
ΔH° for the reaction is +624.7 kJ.
SiO2(g) + 3C(s) → SiC(s) + 2CO(g)
 
  a.   31.2 kJ  
  b.   1.13 × 105 kJv  
  c.   5.06 kJ  
  d.   366 kJ  
  Hint    
      
  9.Calculate the amount of heat absorbed by 10.0 grams of ice at -15.0°C as it is converted to liquid water at 50.0°C. The specific heat of H2O(s) = 2.09 J/(g•°C). The specific heat of H2O(l) = 4.18 J/(g•°C). The heat of fusion is 333 J/g.  
  a.   5.73 kJ  
  b.   2.83 kJ  
  c.   0.676 kJ  
  d.   0.170 kJ  
  Hint    
      
  10.Which of the following occurs with an increase in entropy?  
  a.   the reaction PCl3 (g) + Cl2 (g) → PCl5(g)  
  b.   twenty nickels taken from a box and arranged tails up on a table  
  c.   evaporation of carbon tetrachloride  
  d.   precipitation of silver chloride from a solution of silver ions and chloride ions  
  Hint    
      
  11.At one atmosphere pressure and the melting point of a substance, which statement is true about this general equation?
solid 3 liquid
 
  a.   ΔS = 0 for the process  
  b.   ΔH = 0 for the process  
  c.   Both ΔH and ΔS = 0 for the process  
  d.   ΔG = 0 for the process  
  Hint    
      
  12.For the reaction below, the enthalpy change is +624.7 kJ. How would you classify this reaction?
SiO2(g) + 3C(s) → SiC(s) + 2CO(g)
 
  a.   endothermic reaction, heat is lost from the system  
  b.   exothermic reaction, heat is lost from the system  
  c.   exothermic reaction, heat is gained by the system  
  d.   endothermic reaction, heat is gained by the system  
  Hint    
      
  13.Calculate the enthalpy for the reaction below
2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g)
ΔHf° (kJ/mol) -206.0 0 -348.3 -296.8
 
  a.   -270.6 kJ  
  b.   +270.6 kJ  
  c.   +878.2 kJ  
  d.   -878.2 kJ  
  Hint    
      
  14.A process can never be spontaneous when it is _________.  
  a.   exothermic, and there is an increase in disorder  
  b.   exothermic, and there is an increase in disorder  
  c.   endothermic, and there is an increase in disorder  
  d.   endothermic, and there is a decrease in disorder  
  Hint    
      
  15.In the chemical reaction between aqueous solutions of hydrochloric acid (HCl) and sodium hydroxide (NaOH), what is the chemical system?  
  a.   HCl and water  
  b.   HCl + NaOH → NaCl + H2O  
  c.   NaOH and water  
  d.   aqueous HCl and NaOH  
  Hint    
      
  16.How much heat is required to melt 200 grams of ice? The heat of fusion is 333 J/g.  
  a.   6.66 kJ  
  b.   66.6 kJ  
  c.   1.66 J  
  d.   666 J  
  Hint    
      
  17.Calculate the ΔG° for the reaction below.
2C2H2 (g) + 5O2 (g) → 4CO2 (g) + 2H2O(l)
ΔG° (kJ/mol) 209.2 0 -394.4 -237.2
 
  a.   -1643 kJ  
  b.   -2470 kJ  
  c.   -1409 kJ  
  d.   -2599 kJ  
  Hint    
      
  18.Which of the following substances has an enthalpy value of 0 at 298 K and 1 atmosphere of pressure?  
  a.   HCl(aq)  
  b.   CO2 (g)  
  c.   Na(s)  
  d.   NaOH(s)  
  Hint    
      
  19.The specific heat of aluminum is 0.900 J/(g•°C). How many joules of heat are absorbed by 30.0 g of aluminum if it is heated from 20.0°C to 40.0°C?  
  a.   812 J  
  b.   540 J  
  c.   1.14 × 104 J  
  d.   270 J  
  Hint    
      
  20. From the following data,
H2 (g) + Cl2 (g) → 2HCl(g) ΔH°v = -185 kJ
2H2 (g) + O2 (g) → 2H2O(g) ΔH° = -483.7 kJ
calculate ΔH° for the following reaction.
4HCl(g) + O2 (g) → 2Cl2 (g) + 2H2O(g)
 
  a.   -299 kJ  
  b.   -114 kJ  
  c.   +299 kJ  
  d.   +114 kJ  
  Hint    

 
   
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