   # Assume 3.60 mol of ammonia is placed in a 2.00-L vessel and allowed to decompose to the elements at 723 K. 2 NH 3 (g) ⇄ N 2 (g) + 3 H 2 (g) If the experimental value of K c is 6.3 for this reaction at the temperature in the reactor, calculate the equilibrium concentration of each reagent. What is the total pressure in the flask? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 15, Problem 49GQ
Textbook Problem
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## Assume 3.60 mol of ammonia is placed in a 2.00-L vessel and allowed to decompose to the elements at 723 K.2 NH3(g) ⇄ N2(g) + 3 H2(g)If the experimental value of Kc is 6.3 for this reaction at the temperature in the reactor, calculate the equilibrium concentration of each reagent. What is the total pressure in the flask?

Interpretation Introduction

Interpretation:

The equilibrium concentration of each reagent in the decomposition reaction of ammonia has to be given and the total pressure in the flank has to be determined.

Concept Introduction:

Equilibrium constant in terms of concentration[Kc]: Equilibrium constant can be expressed in terms of concentration.

aA(g)+bB(g)cC(g)+dD(g)Kc=KCc×KDdKAa×KBb

Molarity: It is the number of moles of substance present in a solution of litre.

Molarity =NumberofmolesofsoluteVolumeofsolution(L)

Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

### Explanation of Solution

Given:

2NH3(g)N2(g)+3H2(g)Kc=6.3NumberofmolesofNH3=3.60molV=2L

MolarityofNH3=NumberofmolesVolumeofsolution=3.6mol2L=1.8M

Given the reaction:

2NH3(g)N2(g)+3H2(g)Initialconcentration1.800IfxmolesofammoniareactFinalconcentration1

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