Question:
For the following given equilibrium reaction, K\(_p\) is equal to 1076 at T(K). What is the value of T (in K)?
\[
\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)
\]
Given that \( R = 0.082 \, \text{L atm K}^{-1} \text{mol}^{-1} \), \( K_p = 1076 \), the equation is:
\[
K_p = 1076, \, R = 0.082 \, \text{L atm K}^{-1} \text{mol}^{-1}
\]
For the following given equilibrium reaction, K\(_p\) is equal to 1076 at T(K). What is the value of T (in K)?
\[
\text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g)
\]
Given that \( R = 0.082 \, \text{L atm K}^{-1} \text{mol}^{-1} \), \( K_p = 1076 \), the equation is:
\[
K_p = 1076, \, R = 0.082 \, \text{L atm K}^{-1} \text{mol}^{-1}
\]
Show Hint
The equilibrium constant can be used to calculate temperature or pressure changes at equilibrium by manipulating the Van't Hoff equation.
Updated On: Jun 6, 2025
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The Correct Option is A
Solution and Explanation
We can calculate the temperature (T) using the equation for the equilibrium constant:
\[
K_p = \frac{n_{\text{products}}}{n_{\text{reactants}}} \times e^{-\frac{\Delta H}{RT}}
\]
Substituting the given values, we solve for \( T \). After calculation, the correct temperature is found to be 500 K.
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