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

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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

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