**Equilibrium Constant Problem****Instructions:**Enter your answer in the provided box.**Problem Statement:**For the reaction:\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]Given:- \( K_c \) is 0.393 at 485°C. **Task:**Calculate \( K_p \) for the reaction at this temperature.**Answer Box:**\[ K_p = \underline{\hspace{2cm}} \]**Note:** To calculate \( K_p \), use the relation:\[ K_p = K_c (RT)^{\Delta n} \]Where:- \( R \) = 0.0821 L·atm/mol·K (ideal gas constant)- \( T \) = Temperature in Kelvin (K = °C + 273.15)- \( \Delta n \) = Change in number of moles of gas (products - reactants)Please ensure all substitutions and calculations are clear and accurate before entering your answer.

Answered: Enter your answer in the provided box.…

Enter your answer in the provided box. For the reaction N2(g) + 3H2(g) = 2NH3(g) K, is 0.393 at 485°C. Calculate Kp for the reaction at this temperature. Kp = %3D

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

**Equilibrium Constant Problem**

**Instructions:**
Enter your answer in the provided box.

**Problem Statement:**
For the reaction:

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

Given:
- \( K_c \) is 0.393 at 485°C.

**Task:**
Calculate \( K_p \) for the reaction at this temperature.

**Answer Box:**

\[ K_p = \underline{\hspace{2cm}} \]

**Note:** To calculate \( K_p \), use the relation:
\[ K_p = K_c (RT)^{\Delta n} \]

Where:
- \( R \) = 0.0821 L·atm/mol·K (ideal gas constant)
- \( T \) = Temperature in Kelvin (K = °C + 273.15)
- \( \Delta n \) = Change in number of moles of gas (products - reactants)

Please ensure all substitutions and calculations are clear and accurate before entering your answer.

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