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20 questions
Calculate the value of ΔE in joules for a system that loses 50 J of heat and has 150 J of work performed on it by the surroundings
+200
-100
100
-200
50
The value of ΔH° for the reaction below is -126 kJ. _____ kJ are released when 2.00 mol of NaOH is formed in the reaction?
63
252
3.9
-126
7.8
The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is ____ kJ.
-12
-790
-23
23
12
The value of ΔH° for the reaction below is +128.1 kJ. How many kJ of heat are consumed when 5.10 g of H2 (g) is formed as shown in the equation?
653
326
162
128
62.0
° The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 ° C to 37 °C .
0.00054
29
0.13
-0.13
2.0
The specific heat of bromine liquid is 0.226 J/g-K. The molar heat capacity (in J/mol-K) of bromine liquid is ____.
707
0.226
9.05
36.1
18.1
° The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C ? The density of liquid bromine: 3.12 g/mL.
5.20
16.2
32.4
10.4
300
Given the data in the table above, ΔHrxn° for the reaction is ______ kJ.
-1892
-1172
-150
-1540
Given the data in the table above, ΔH°rxn for the reaction is _____________ kJ.
-3.2
-1.6
1.6
3.2
ΔH for the reaction is ____ kJ.
-1135
1135
35
-35
355
Given the following reactions the enthalpy of the reaction of the nitrogen to produce nitric oxide is ____ kJ.
180.6
-180.6
90.3
-47.8
47.8
A 25.5 g piece of cheddar cheese contains 37% fat, 28% protein and 4% carbohydrate. The respective fuel ratios are 38, 17 and 17 kJ/g. What is the fuel value for this piece of cheese in kJ?
99
500
260
330
790
Which one of the following conditions would always result in an increase in the internal energy of a system?
The system gains heat and has work done on it by the surroundings
The system gains heat and does work on the surroundings
The system loses heat and does work on the surroundings
The system loses heat and has work done on it by the surroundings
None of the above
Which of the following statements is false?
The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction
The enthalpy of a reaction is equal to the heat of the reaction
Enthalpy is an intensive property
Internal energy is a state function
The enthalpy change for a reaction depends on the state of the reactants and products
The combustion of titanium with oxygen produces titanium dioxide. When 2.060 g of titanium is combusted in a bomb calorimete, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C . In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimter is _____ kJ/mol.
19.6
-0.154
-0.000152
14.3
-311
For the reaction of ethylene represented below, ΔH is -1323 kJ. What is the value of ΔH if the combustion produced liquid water rather than water vapor? ( ΔH for the phase change H2O (g) → H2O (l) is -44 kJ/mol).
-1235 kJ
-1279 kJ
-1367 kJ
-1411 kJ
For the reaction above, what is the energy change when 0.50 moles of C2H5OH are reacted?
277.7 kJ
138.8 kJ
-138.8 kJ
-555.4 kJ
What is the change in internal energy, ΔE , for a system that does 70 J of work as it absorbs 45 J of heat.
115 J
25 J
-25 J
-115 J
Which of these species has a standard enthalpy of formation of zero?
F2 (g)
F (g)
HF (aq_
F- (aq)
Given the data in the table below, ΔH°rxn for the reaction is ______ kJ.
-3.2
-1.6
+1.6
+3.2
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