The equilibrium constant, Kc, for the following reaction is 7.00 × 10-5 at 673 K. NH₂I(s) ⇒ NH3 (g) + HI(g) If an equilibrium mixture of the three compounds in a 5.07 L container at 673 K contains 3.24 mol of NH₂I(s) and 0.473 mol of NH3, the number of moles of HI present is mol.
The equilibrium constant, Kc, for the following reaction is 7.00 × 10-5 at 673 K. NH₂I(s) ⇒ NH3 (g) + HI(g) If an equilibrium mixture of the three compounds in a 5.07 L container at 673 K contains 3.24 mol of NH₂I(s) and 0.473 mol of NH3, the number of moles of HI present is mol.
Chemistry
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Chapter1: Chemical Foundations
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![**Problem Statement:**
Use the References to access important values if needed for this question.
The equilibrium constant, \( K_c \), for the following reaction is \( 7.00 \times 10^{-5} \) at 673 K.
\[ \text{NH}_4\text{I}_{(s)} \rightleftharpoons \text{NH}_3_{(g)} + \text{HI}_{(g)} \]
If an equilibrium mixture of the three compounds in a 5.07 L container at 673 K contains 3.24 mol of \(\text{NH}_4\text{I}\) and 0.473 mol of \(\text{NH}_3\), the number of moles of \(\text{HI}\) present is \(\_\_\_\_\_\) mol.
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**Explanation:**
This problem involves calculating the equilibrium concentrations of species in a chemical reaction. Given \( K_c \), the volume of the container, and initial moles of two reactants/products, we need to find the moles of the remaining species at equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffb429895-490e-408d-91b7-04d28a4f9844%2Fd1f8f0af-9085-4994-b726-85a59dc299d1%2F2a99djg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Use the References to access important values if needed for this question.
The equilibrium constant, \( K_c \), for the following reaction is \( 7.00 \times 10^{-5} \) at 673 K.
\[ \text{NH}_4\text{I}_{(s)} \rightleftharpoons \text{NH}_3_{(g)} + \text{HI}_{(g)} \]
If an equilibrium mixture of the three compounds in a 5.07 L container at 673 K contains 3.24 mol of \(\text{NH}_4\text{I}\) and 0.473 mol of \(\text{NH}_3\), the number of moles of \(\text{HI}\) present is \(\_\_\_\_\_\) mol.
**Actions:**
- Submit Answer
- Retry Entire Group
**Remaining Attempts:** 9 more group attempts remaining
**Explanation:**
This problem involves calculating the equilibrium concentrations of species in a chemical reaction. Given \( K_c \), the volume of the container, and initial moles of two reactants/products, we need to find the moles of the remaining species at equilibrium.
Expert Solution
Step 1: Defining equilibrium constant!
Answer:
For any given reaction, value of equilibrium constant KC is equal to the ratio of molar concentrations of product and reactant gases at equilibrium.
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