A student ran the following reaction in the laboratory at 759 K:\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]When she introduced \( 3.13 \times 10^{-2} \) moles of \(\text{N}_2(g)\) and \( 6.00 \times 10^{-2} \) moles of \(\text{H}_2(g)\) into a 1.00 liter container, she found the equilibrium concentration of \(\text{NH}_3(g)\) to be \( 6.84 \times 10^{-4} \, \text{M} \).Calculate the equilibrium constant, \( K_c \), she obtained for this reaction.\[ K_c = \]

Answered: A student ran the following reaction in…

Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Question

A student ran the following reaction in the laboratory at 759 K:

\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]

When she introduced \( 3.13 \times 10^{-2} \) moles of \(\text{N}_2(g)\) and \( 6.00 \times 10^{-2} \) moles of \(\text{H}_2(g)\) into a 1.00 liter container, she found the equilibrium concentration of \(\text{NH}_3(g)\) to be \( 6.84 \times 10^{-4} \, \text{M} \).

Calculate the equilibrium constant, \( K_c \), she obtained for this reaction.

\[ K_c = \]

Expert Solution

Introduction

One or more substances that are involved in a chemical or biochemical reaction are referred to as reactants or substrates. One or more substances that are produced after a reaction is referred to as products.

A reversible chemical reaction in which reactants and products are stable at both ends is referred to as an equilibrium reaction. In such a reaction, no net change between the number of reactants and products are involved.