Chemistry: Matter and Change

Chapter 15: Energy and Chemical Change

Standardized Test Practice

1
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)540 J
B)270 J
C)812 J
D)1.14 x 104 J
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)25°C
B)30°C
C)35°C
D)40°C
3
If a 1 kg granite slab is heated from 0.0 degrees C to 25 degrees C, how much heat in Joules does it absorb?

<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=jpg::::/sites/dl/free/007874637x/514791/tab15_2.jpg','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (32.0K)</a>
A)3.1 x 104 J
B)2.5 x 104 J
C)2.0 x 104 J
D)2.5 J
4
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)endothermic reaction, heat is gained by the system
C)exothermic reaction, heat is lost from the system
D)exothermic reaction, heat is gained by the system
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)96.3 kJ
B)192 kJ
C)289 kJ
D)460 kJ
6
In the hot pack process, 1625 kJ of heat is released to the surroundings for each 2 moles of Fe2O3 produced. Find the heat released if 50.0 grams of Fe2O3 are produced.

4Fe(s) + 3O2(g) → 2Fe2O3(s) + 1625 kJ
A)508 kJ
B)245 kJ
C)254 kJ
D)805 kJ
7
How much heat is required to melt 200 grams of ice? The molar enthalpy (heat) of fusion is -6.01 kJ/mol.
A)66.7 kJ
B)667 J
C)1.66 J
D)6.66 kJ
8
Find the heat released by the combustion of 1.00 grams of table sugar.

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A)5.66 kJ
B)16.5 kJ
C)5644 kJ
D)194 kJ
9
The water vapor escaping from microwave popcorn can be dangerous. Find the heat released if 1.00 gram of water condenses from vapor.

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A)9.04 kJ
B)4.52 kJ
C)2.26 kJ
D)1.13 kJ
10
Hess's law can be used to ________.

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A)calculate the energy change for reactions for which it is impractical or impossible to measure delta H
B)calcualte the energy change for reactions that happen only in a laboratory
C)calculate the energy change for reactions for which the heat produced is too great to measure in a laboratory
D)calculate the energy change for reactions that do not obey the Second Law of Thermodynamics.
11
Given the following information,
SO3 (g) + H2O(l) → H2SO4 (l) ΔH° = -133 kJ, Pb(s) + PbO2 (s) + 2H2SO4(l) → 2PbSO4(s) + 2H2O(l) ΔH° = -509 kJ,
calculate the ΔH° for the reaction below.

Pb(s) + PbO2 (s) + 2SO3 (g) →2PbSO4 (s)
A)376 kJ
B)-376 kJ
C)-642 kJ
D)-775 kJ
12
Calculate ΔH° for the following reaction. The standard enthalpies of formation for the two reactants and two products are, in order, -206.0, 0, -348.3, -296.8

2ZnS(s) + 3O2(g) → 2ZnO (s) + 2SO2(g)
A)-270.6 kJ
B)-878.2 kJ
C)+270.6 kJ
D)+878.2 kJ
13
A process can never be spontaneous when it is _________.
A)exothermic, and there is an increase in disorder
B)endothermic, and there is an increase in disorder
C)exothermic, and there is a decrease in disorder
D)endothermic, and there is a decrease in disorder
14
In which of the following everyday situations does the entropy of the system decrease?
A)An egg breaks on the floor.
B)Sugar dissolves in tea.
C)Frost forms on grass.
D)A building is knocked over in a storm.
15
For a particular process, ΔHsystem = 60 kJ and ΔSsystem = 200 J/K. Find ΔGsystem at 298 K. Is the process spontaneous?

ΔGsystem = ΔHsystem - TΔSsystem
A)-0.4 kJ, spontaneous
B)-0.4 kJ, nonspontaneous
C)0.4 kJ, spontaneous
D)0.4 kJ, nonspontaneous
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