Explanation Given: To calculate equilibrium constant at given reaction are, B r 2 ( g ) + C l 2 ( g ) ⇌ 2 B r C l ( g ) B r C l = − 0.1 k J / m o l Formula Used: ( i ) Δ G r x n 0 = ∑ n p Δ G f 0 ( p r o d u c t ) − ∑ n r Δ G f 0 ( r e a c tan t ) ( i i ) Δ G r x n 0 = − R T ln K R i s t h e g a s c o n s t a n t , T i s t e m p e r a t u r e a t 298 k , k p i s t h e e q u i l i b r i u m f r o m t h e p a r t i a l p r e s s u r e ...

Chemistry: Structure and Properties (2nd Edition)

2nd Edition

ISBN: 9780134293936

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 18, Problem 74E

Interpretation Introduction

(b)

To determine:

The equilibrium constant at 25⁰C for the reaction:

$B r_{2}_{(g)} + C l_{2}_{(g)} ⇌ 2 B r C l_{(g)}$

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Chapter 18, Problem 73E

Chapter 18, Problem 75E

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Chapter 18 Solutions

Chemistry: Structure and Properties (2nd Edition)

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(b) To determine: The equilibrium constant at 25 0 C for the reaction: B r 2 ( g ) + C l 2 ( g ) ⇌ 2 B r C l ( g )

Solution Summary: The author explains how to calculate the equilibrium constant at 25 0 C for the reaction 2 N O 2 N 2 O 4.

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(b)

To determine:

The equilibrium constant at 25⁰C for the reaction:

$B r_{2}_{(g)} + C l_{2}_{(g)} ⇌ 2 B r C l_{(g)}$

Want to see the full answer?

Chapter 18 Solutions

(b) To determine: The equilibrium constant at 25 0 C for the reaction: B r 2 ( g ) + C l 2 ( g ) ⇌ 2 B r C l ( g )

Solution Summary: The author explains how to calculate the equilibrium constant at 25 0 C for the reaction 2 N O 2 N 2 O 4.

Videos

(b) To determine: The equilibrium constant at 250C for the reaction: Br2(g)+Cl2(g)⇌2BrCl(g)

Want to see the full answer?

Chapter 18 Solutions

(b)

To determine:

The equilibrium constant at 25⁰C for the reaction:

$B r_{2}_{(g)} + C l_{2}_{(g)} ⇌ 2 B r C l_{(g)}$