What is the value of ∆G°(kJ mol–1 ) for this reaction at 175.4 oC ? The data refer to 25 oC: 2 NO(g) + Cl2(g) ⟶ 2 NOCl(g)SubstanceNO(g)Cl2(g)NOCl(g)∆H°f (kJ mol–1)90.29051.71∆G°f (kJ mol–1)86.60066.07S° (J K–1 mol–1)210.65223.0261.6 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) Calculate ΔG in kJ•mol-1 at 298 K for the following reaction: under the following conditions: (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)P(A) = 0.397 atm, P(AB) = 0.792 atm2 A(g) + B2(s) → 2 AB(g) ΔGo = -182 kJ•mol-1 The redox reaction below has a ΔG° value of 209. kJ. Determine the standard cell potential(E°cell) for this reaction.A2+(aq) + 2B2+(aq) → A4+(aq) + 2B+(aq) Need help with these 3 asap excuse the numbers

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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

Section: Chapter Questions

Problem 68SCQ: Explain why each of the following statements is incorrect. (a) Entropy increases in all spontaneous...

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What is the value of ∆G°(kJmol^–1) for this reaction at 175.4 ^oC ? The data refer to 25 ^oC:

2 NO(g) + Cl₂(g) ⟶ 2 NOCl(g)

Substance	NO(g)	Cl₂(g)	NOCl(g)
∆H°_f (kJ mol^–1)	90.29	0	51.71
∆G°_f (kJ mol^–1)	86.60	0	66.07
S° (J K^–1 mol^–1)	210.65	223.0	261.6

(the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)

Calculate ΔG in kJ•mol^-1 at 298 K for the following reaction: under the following conditions:
(the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)
P(A) = 0.397 atm, P(AB) = 0.792 atm
2 A(g) + B2(s) → 2 AB(g) ΔG^o = -182 kJ•mol^-1

The redox reaction below has a ΔG° value of 209. kJ. Determine the standard cell potential(E°_cell) for this reaction.

A²⁺(aq) + 2B²⁺(aq) → A⁴⁺(aq) + 2B⁺(aq)

Need help with these 3 asap excuse the numbers

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