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1		A system expands in volume from 2.0 L to 24.5 L at constant temperature. Calculate the work (w) if the expansion occurs against a constant pressure of 5.00 atm.
			A)	-113 J
			B)	1.24 x 104 J
			C)	-1.14 x 104 J
			D)	113 J
			E)	1.14 x 104 J
2		If 1700 cal of heat is added to a system while the system does work equivalent to 3000 cal by expanding against the surrounding atmosphere, the value of ΔE for the process is
			A)	-1300 cal
			B)	4700 cal
			C)	1300 cal
			D)	-4700 cal
			E)	2350 cal
3		Which of the following is not a state function?
			A)	ΔE
			B)	ΔH
			C)	q
			D)	P
			E)	V
4		In which one of the following processes is ΔH = ΔE?
			A)	2HI(g) → H2(g) + I2(g) at atmospheric pressure.
			B)	Two moles of ammonia gas are cooled from 325 °C to 300 °C at 1.2 atm.
			C)	H2O(l) → H2O(g) at 100 °C at atmospheric pressure.
			D)	CaCO3(s) → CaO(s) + CO2(g) at 800 °C at atmospheric pressure.
			E)	CO2(s) → CO2(g) at atmospheric pressure.
5		Data: (1)   H2(g) + ½O2(g) → H2O(g)   ΔH = -241.8 kJ (2)  H2(g) + ½O2(g) → H2O(l)   ΔH = -285.8 kJ On the basis of the above data, which of the following statements is false?
			A)	Reaction (1) is exothermic.
			B)	Reaction (2) is the formation reaction for H2O(l).
			C)	The reverse of reaction (2) is endothermic.
			D)	The energy content of H2O(g) is lower than H2O(l).
			E)	ΔH for the reaction: H2O(l) → H2O(g) is + 44 kJ/mol.
6		On a gram for gram basis, which of the following substances will release the most energy when it is burned?
			A)	<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=gif:: ::/sites/dl/free/0072396814/37547/Image1.gif','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (1.0K)</a>
			B)	<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=gif:: ::/sites/dl/free/0072396814/37547/Image2.gif','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (1.0K)</a>
			C)	<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=gif:: ::/sites/dl/free/0072396814/37547/Image3.gif','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (1.0K)</a>
			D)	<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=gif:: ::/sites/dl/free/0072396814/37547/Image4.gif','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (1.0K)</a>
			E)	<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=gif:: ::/sites/dl/free/0072396814/37547/Image5.gif','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (1.0K)</a>
7		What is the amount of heat necessary to raise the temperature of 8.5 kg of water from 12.5 °C to 84 °C?
			A)	3.0 x 103 kJ
			B)	36 J
			C)	2.5 x 103 kJ
			D)	2.5 x 106 kJ
			E)	25 kJ
8		When 50. mL (50. g) of 1.00 M HCl at 22.00 °C is added to 50. mL (50. g) of 1.00 M NaOH at 22.00 °C in a coffee cup calorimeter, the temperature increases to 28.87 °C. What is the heat (q) of the reaction between HCl and NaOH? (The specific heat of the solution produced is 4.18 J/g·°C.)
			A)	-6.3 x 103 J
			B)	-3.2 x 103 J
			C)	-2.9 x 103 J
			D)	-1.7 x 103 J
			E)	-1.4 x 103 J
9		A hydrocarbon sample was burned in a bomb calorimeter. The temperature of the calorimeter and the 1.00 kg of water rose from 20.45 °C to 23.65 °C. The heat capacity of the calorimeter, excluding the water, is 2.21 kJ/°C. Using this information, determine the heat released by the combustion.
			A)	13.3 kJ
			B)	20.5 kJ
			C)	46.0 kJ
			D)	86.8 kJ
			E)	none of the above
10		Data:  SO2(g) + ½O2(g) → SO3(g)   ΔH° = -99kJ Use the data above to calculate the standard enthalpy change for the reaction below. Reaction: 2SO3(g) → O2(g) + 2SO2(g)   ΔH° = ?
			A)	99 kJ
			B)	-198 kJ
			C)	49.5 kJ
			D)	-99 kJ
			E)	198 kJ
11		Data:  SO2(g) + ½O2(g) → SO3(g)   ΔH = -99.1 kJ Given the above data, calculate the enthalpy change ΔH when 89.6 g of SO2 is converted to SO3.
			A)	-69.3 kJ
			B)	-139 kJ
			C)	69.3 kJ
			D)	139 kJ
			E)	-111 kJ
12		Data: C(graphite) + O2(g) → CO2(g)   ΔH° = -393.5 kJ H2(g) + ½O2(g) → H2O(l)   ΔH° = -285.8 kJ CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l)   ΔH° = -726.4 kJ Using the data above, calculate the enthalpy change for the reaction below. Reaction: C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l)
			A)	+238.7 kJ
			B)	-238.7 kJ
			C)	+548.3 kJ
			D)	-548.3 kJ
			E)	+904.5 kJ
13		Data: 2Ba(s) + O2(g) → 2BaO(s)    ΔH° = -1107.0 kJ Ba(s) + CO2(g) + ½O2(g) → BaCO3(s)   ΔH° = -822.5 kJ Given the data above, calculate ΔH° for the reaction below. Reaction: BaCO3(s) → BaO(s) + CO2(g)
			A)	-1929.5 kJ
			B)	-1376.0 kJ
			C)	-284.5 kJ
			D)	269.0 kJ
			E)	537 kJ
14		Which one of the following reactions occurring at 25 °C is the formation reaction of H2SO4(l)?
			A)	H2(g) + S(s) + 2O2(g) → H2SO4(l)
			B)	H2SO4(l) → H2(g) + S(s) + 2O2(g)
			C)	H2(g) + S(g) + 2O2(g) → H2SO4(l)
			D)	H2SO4(l) → 2H(g) + S(s) + 4O(g)
			E)	2H(g) + S(g) + 4O(g) → H2SO4(l)
15		Data:  ΔH°f values: CH4(g), -74.8 kJ; CO2(g), -393.5 kJ; H2O(l), -285.8 kJ. Using the ΔH°f data above, calculate ΔH°rxn for the reaction below. Reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
			A)	-604.2 kJ
			B)	890.3 kJ
			C)	-997.7 kJ
			D)	-890.3 kJ
			E)	none of the above