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Home  arrow Chapter 5: Thermochemistry  arrow Quiz 1

Quiz 1



This activity contains 12 questions.

Question 1.

Substance delta.gifHf° (kJ/mol)
SO2(g) -297
SO3(g) -396
SO2Cl2(g) -364
H2SO4(l) -814
H2O(l) -286

Determine the value of delta.gif in kJ for the following reaction:
2SO2(g) + O2(g) --> 2SO3(g)

 
End of Question 1


Question 2.

Calculate H° for the following reaction, using the given enthalpies of formation.

2NO(g) + O2(g) --> 2NO2(g)

Hf[NO(g)] = 90.25 kJ mol-1

Hf[NO2(g)] = 33.18 kJ mol-1

 
End of Question 2


Question 3.

Consider the combustion reaction of ethane gas, C2H6(g):

C2H6(g) + 7/2O2(g) --> 2CO2(g) + 3H2O(g) H = -1430 kJ

What is the enthalpy change for the reverse reaction if whole-number coefficients are used?

 
End of Question 3


Question 4.

Consider the reaction

Pb2+(aq) + 2Cl-(aq) --> PbCl2(s) H = -22.53 kJ/mol

Calculate H when 0.230 mol of PbCl2(s) is dissolved in water.

 
End of Question 4


Question 5.

From the following heats of reaction,

2C (graphite) + H2 (g) --> C2H2 (g) H = 227 kJ

6C (graphite) + 3H2 (g) --> C6H6 (l) H = 49 kJ

calculate the heat for the reaction

3C2H2 (g) --> C6H6 (l)

 
End of Question 5


Question 6.
How many kJ of heat must be removed from 1000. g of water (heat capacity of 4.184 J g-1 K-1) to lower the temperature from 18.0°C to 12.0°C?

 
End of Question 6


Question 7.
How much heat in kJ is required to raise the temperature of 125 g H2O from 2.2°C to 48.6°C? (The specific heat of water is 4.18 J g-1 °C-1.)

 
End of Question 7


Question 8.
Of the substances below, which one has the highest fuel value?

 
End of Question 8


Question 9.
The heat of combustion of fructose, C6H12O6(s), is -2812 kJ/mol. Using the information in Table 5.3, calculate f for fructose.

 
End of Question 9


Question 10.

Use the delta.gifH values for equations 1 and 2 to determine the value of delta.gifH for equation 3.
(1) 2NO --> N2 + O2 delta.gifH = -180 kJ
(2) 2NO + O2 --> 2NO2 delta.gifH = -112 kJ
(3) N2 + 2O2 --> 2NO2 delta.gifH = ?
 
End of Question 10


Question 11.

Use the following thermochemical equations

C2H5OH (l) + 3O2(g) --> 2CO2 (g) + 3H2O (l) H° = -1367 kJ

H2(g) + 1/2 O2(g) --> H2O(l) H° = -286 kJ

C (graphite) + O2(g) --> CO2(g) H° = -394 kJ

to calculate the enthalpy change for the following reaction:

2C (g) + 3H2 (g) + 1/2O2 (g) --> C2H5OH (l) H° = ?

 
End of Question 11


Question 12.
Which of the following is not a state function?

 
End of Question 12





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