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.

(a) The desired equation to calculate the ΔH is: 8Ni (s) + S8(s) + 12O2 (g) → 8NiSO3 (s)∆H (in kJ) for the reaction can be calculated as follows: ∆H = 4 ∆H3 - 8∆H1 - 8∆H2 8 Ni (s) + 4O2 (g) →8NiO (s) ∆H = 4×(-478)kJ.S8 (s) + 8O2 (g) →8 SO2 (g) ∆H = 8×(-290)kJ.8NiO (s) + 8 SO2 (g)→ 8NiSO3 (s) ∆H = 8×(-162)kJ.8 Ni (s) +S8 (s) + 12O2 (g) → 8NiSO3 (s)∆H =4×(-478)+ 8×(-290)+ 8×(-162)=-5528 KJ. (b) If the reaction is reversed ∆H will change its sign. 8 NiSO3 (s) 8 Ni (s) + S8(s) + 12 O2(g) ; ∆H = + 5528.0 KJ Mass of NiSO3 = 2.0 g Molar mass of NiSO3 = 138.76 g/mol Moles of NiSO3 = 2.0 / 138.76 = 0.0144 mol. From the balanced equation, 8 mol NiSO3 ____________ 5528 KJ 0.0144 mol NiSO3 ___________ ? ∆H for the decomposition of NiSO3 = ∆H=0.0144×55288=9.95 KJ.(c) The molar heat capacity = 131.3 J/mol 0C. Mass = 22 g. ΔT = 66 – 22 = 44 0C. The number of moles of CCl4 = 22/153.82 mol. The amount of energy required = q = n Cp∆Tq= 22153.82×131.3×44=826.28 J.=0.82628 kJ.

Answered: Consider the following reactions.…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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)

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)

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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