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Calculate ΔrH° (in  kJ mol−1), ΔrS° (in J K−1 mol−1),  ΔrG° (in kJ mol−1) at 298.15 K for the reaction below.       C(gr.) + 12 N2(g) + 52 H2(g) ⟶ CH3NH2(g) ΔfH ° at 298.15 K / kJ mol−1 0   0   0   −22.97 S¯ ∘at 298.15 K / J K−1 mol−1 5.74   191.61   130.68

Calculate ΔrH° (in  kJ mol−1), ΔrS° (in J K−1 mol−1),  ΔrG° (in kJ mol−1) at 298.15 K for the reaction below.       C(gr.) + 12 N2(g) + 52 H2(g) ⟶ CH3NH2(g) ΔfH ° at 298.15 K / kJ mol−1 0   0   0   −22.97 S¯ ∘at 298.15 K / J K−1 mol−1 5.74   191.61   130.68

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section18.5: Entropy Changes And Spontaneity
Problem 1RC
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Calculate ΔrH° (in  kJ mol−1), ΔrS° (in J K−1 mol−1),  ΔrG° (in kJ mol−1) at 298.15 K for the reaction below.  

 

  C(gr.) + 12 N2(g) + 52 H2(g) ⟶ CH3NH2(g)

ΔfH ° at 298.15 K

/ kJ mol−1

 0   0   0   −22.97

S¯ ∘at 298.15 K

/ J K−1 mol−1

 5.74   191.61   130.68   243.4

 

Give your answers in the specified units. Please double check your solution.

 

 

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