Consider the following reactions. NiSO3(s) →NiO (s) + SO2 (g)        ∆H= 162.0 kJ   SO2 (g) →   1/8 S8(s) + O2 (g)      ∆H= 290.0 kJ     2Ni (s) + O2 (g) → 2NiO (s)          ∆H= -478.0 kJ   A) Calculate ∆H (in kJ) for the reaction. 8Ni (s) + S8(s) + 12O2 (g) →8NiSO3 (s) B) Calculate ∆H (in kJ) for the decomposition reaction of 2.00 g of NiSO3(s) according to the reaction.            8NiSO3 (s)→ 8Ni (s) + S8(s) + 12O2 (g)   C) Carbon tetrachloride (CCl4) was at one time used as a fire-extinguishing agent. The molar heat capacity is 131.3 J/(mol°C). Calculate the amount of energy in kJ required to raise the temperature of 22.0 g of CCl4 from 22.0 °C to 66.0 °C.

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Chapter6: Thermochemistry
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Problem 111AE: At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/mol and 49 kJ/mol,...
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Consider the following reactions.

  1. NiSO3(s) →NiO (s) + SO2 (g)        ∆H= 162.0 kJ

 

  1. SO2 (g) →   1/8 S8(s) + O2 (g)      ∆H= 290.0 kJ

 

 

  1. 2Ni (s) + O2 (g) → 2NiO (s)          ∆H= -478.0 kJ

 

A) Calculate ∆H (in kJ) for the reaction.

8Ni (s) + S8(s) + 12O2 (g) →8NiSO3 (s)

B)

Calculate ∆H (in kJ) for the decomposition reaction of 2.00 g of NiSO3(s) according to the reaction.

          

8NiSO3 (s)→ 8Ni (s) + S8(s) + 12O2 (g)

 

C)

Carbon tetrachloride (CCl4) was at one time used as a fire-extinguishing agent.

The molar heat capacity is 131.3 J/(mol°C). Calculate the amount of energy in kJ required to raise the temperature of 22.0 g of CCl4 from 22.0 °C to 66.0 °C.

 

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