For the reaction2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (g)AH° -81.1 kJ and AS⁰ = - - 1.20 J/KThe equilibrium constant for this reaction at 308.0 K isAssume thatΔΗ° andAS are independent of temperature. For the reactionN₂ (g) + O₂(g) → 2NO(g)181 kJ and AS⁰ =24.9 J/KThe equilibrium constant for this reaction at 327.0 K isΔΗ° =Assume thatΔΗ° andAS are independent of temperature.

The objective of the question is to calculateThe equilibrium constant for the reaction at .The…

For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH = -81.1 kJ and AS = -1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.

For the reaction 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH = -81.1 kJ and AS = -1.20 J/K The equilibrium constant for this reaction at 308.0 K is Assume that ΔΗ° and AS are independent of temperature.

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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Question

For the reaction
2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂ (g)
AH° -81.1 kJ and AS⁰ = - - 1.20 J/K
The equilibrium constant for this reaction at 308.0 K is
Assume that
ΔΗ° and
AS are independent of temperature.

For the reaction
N₂ (g) + O₂(g) → 2NO(g)
181 kJ and AS⁰ =
24.9 J/K
The equilibrium constant for this reaction at 327.0 K is
ΔΗ° =
Assume that
ΔΗ° and
AS are independent of temperature.

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