Multiple Choice 1.How much heat is released when 1.0 mol of HBr is formed in this reaction: H2 (g) + Br2(g) → 2HBr(g). The value of ΔH0 for the reaction is -72 kJ. A. 72 B. 44 C. 36 D. -72 2. The value of ΔH0for the reaction is -126 kJ. Determine the heat released when 2.00 mol of NaOH is formed in the reaction: 2Na2O2 (s) + 2H2O (l) → 2NaOH(s) + O2 (g) inn kJ. A. 252 B. 63 C. 3.9 D. 7.8 3.The value of ΔH0for the reaction is -790 kJ. What is the enthalpy change accompanying the reaction of 0.95 g of S in kJ: 2S(s) + 3O2(g) → 2SO3(g). A. 23 B. -23 C. -12 D. 12 4. The value of ΔH0for the reaction is -6535 kJ. What is the heat released in the combustion of 16.0 g of C6H6(l): 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) in kJ? A. 1.3x103 B. 5.23x104 C. 669 D. 2.68x103 5. The enthalpy change for the reaction: 2H2(g)+ O2(g) → 2H2O(g) is -483.6 kJ. Determine the enthalpy change for the reaction: 4H2(g) + 2O2(g) → 4H2O(g) in kJ. A. -483.6 B. -967.2 C. 483.6 D. 967.2 6. The value of ΔH0for the reaction CH3OH(l) → CO(g) + 2H2(g) is +128.1 kJ. Determine the heat consumed when 15.5 g of CH3OH(l) decomposes. A. 0.48 B. 62.0 C. 32 D. 8.3 7. Which of the following is a statement of the first law of thermodynamics? A. Ek= ½ mv2 B. A negative ΔH corresponds to an exothermic process. C. ΔE = Efinal – Einitial D. Energy lost by the system must be gained by the surroundings. 8. The reaction: 4Al(s) + 3O2(g) → 2Al2O3(s); ΔH0= -3351 kJ, the reaction is ___________, and therefore heat is __________ by the reaction. A. endothermic, released B. endothermic, absorbed C. exothermic, released D. exothermic, absorbed
Multiple Choice
1.How much heat is released when 1.0 mol of HBr is formed in this reaction: H2 (g) + Br2(g) → 2HBr(g). The value of ΔH0 for the reaction is -72 kJ.
A. 72
B. 44
C. 36
D. -72
2. The value of ΔH0for the reaction is -126 kJ. Determine the heat released when 2.00 mol of NaOH is formed in the reaction: 2Na2O2 (s) + 2H2O (l) → 2NaOH(s) + O2 (g) inn kJ.
A. 252
B. 63
C. 3.9
D. 7.8
3.The value of ΔH0for the reaction is -790 kJ. What is the enthalpy change accompanying the reaction of 0.95 g of S in kJ: 2S(s) + 3O2(g) → 2SO3(g).
A. 23
B. -23
C. -12
D. 12
4. The value of ΔH0for the reaction is -6535 kJ. What is the heat released in the combustion of 16.0 g of C6H6(l): 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) in kJ?
A. 1.3x103
B. 5.23x104
C. 669
D. 2.68x103
5. The enthalpy change for the reaction: 2H2(g)+ O2(g) → 2H2O(g) is -483.6 kJ. Determine the enthalpy change for the reaction: 4H2(g) + 2O2(g) → 4H2O(g) in kJ.
A. -483.6
B. -967.2
C. 483.6
D. 967.2
6. The value of ΔH0for the reaction CH3OH(l) → CO(g) + 2H2(g) is +128.1 kJ. Determine the heat consumed when 15.5 g of CH3OH(l) decomposes.
A. 0.48
B. 62.0
C. 32
D. 8.3
7. Which of the following is a statement of the first law of
A. Ek= ½ mv2
B. A negative ΔH corresponds to an exothermic process.
C. ΔE = Efinal – Einitial
D. Energy lost by the system must be gained by the surroundings.
8. The reaction: 4Al(s) + 3O2(g) → 2Al2O3(s); ΔH0= -3351 kJ, the reaction is ___________, and therefore heat is __________ by the reaction.
A. endothermic, released
B. endothermic, absorbed
C. exothermic, released
D. exothermic, absorbed
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