**Consider the Reaction**\[ \text{A(aq)} \rightleftharpoons 2\text{B(aq)} \]\[K_c = 4.46 \times 10^{-6} \text{ at 500 K}\]**Problem Statement:**If a 4.70 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?**Solution:**\[[B] = \_\_\_\_\_\_\_ \text{ M}\]**Explanation:**The problem involves calculating the concentration of B in a chemical equilibrium using the given equilibrium constant \( K_c \) and the initial concentration of A. The equilibrium constant \( K_c \) provides the ratio of the concentrations of products to reactants at equilibrium at a given temperature (500 K in this case). The process involves setting up an equilibrium table (ICE table), calculating changes in concentration using stoichiometry, and applying the equilibrium expression. This is a typical example of a chemical equilibrium problem often encountered in chemistry courses.

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Answered: Consider the reaction. A(aq) =2 B(aq)…

Consider the reaction. A(aq) =2 B(aq) K. = 4.46 x 10-6 at 500 K If a 4.70 M sample of A is heated to 500 K, what is the concentration of B at equilibrium? B] =

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

**Consider the Reaction**

\[ \text{A(aq)} \rightleftharpoons 2\text{B(aq)} \]

\[
K_c = 4.46 \times 10^{-6} \text{ at 500 K}
\]

**Problem Statement:**

If a 4.70 M sample of A is heated to 500 K, what is the concentration of B at equilibrium?

**Solution:**

\[
[B] = \_\_\_\_\_\_\_ \text{ M}
\]

**Explanation:**

The problem involves calculating the concentration of B in a chemical equilibrium using the given equilibrium constant \( K_c \) and the initial concentration of A.

The equilibrium constant \( K_c \) provides the ratio of the concentrations of products to reactants at equilibrium at a given temperature (500 K in this case). The process involves setting up an equilibrium table (ICE table), calculating changes in concentration using stoichiometry, and applying the equilibrium expression.

This is a typical example of a chemical equilibrium problem often encountered in chemistry courses.

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