Suppose a 250. mL flask is filled with 0.10 mol of H₂ and 1.8 mol of I2. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.948 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places. M S ?
Suppose a 250. mL flask is filled with 0.10 mol of H₂ and 1.8 mol of I2. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.948 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places. M S ?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 121QRT: When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above...
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![**Chemical Equilibrium Problem**
**Introduction:**
Consider a 250 mL flask filled with 0.10 mol of hydrogen gas (H₂) and 1.8 mol of iodine gas (I₂). The following reaction can occur:
\[ \text{H}_2(\text{g}) + \text{I}_2(\text{g}) \rightleftharpoons 2\text{HI}(\text{g}) \]
**Equilibrium Constant:**
The equilibrium constant, \( K \), for this reaction is 0.948 at the temperature of the flask.
**Problem Statement:**
Calculate the equilibrium molarity of hydrogen iodide (HI). Round your answer to two decimal places.
**Input Field:**
\[ \boxed{ \_\_ \text{M} } \]
**Submission Buttons:**
- A checkmark (✔️) for submitting the answer.
- A counterclockwise arrow (](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2F1b4d5264-a417-4562-8e27-d0ecd33e3e85%2Fa772acb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium Problem**
**Introduction:**
Consider a 250 mL flask filled with 0.10 mol of hydrogen gas (H₂) and 1.8 mol of iodine gas (I₂). The following reaction can occur:
\[ \text{H}_2(\text{g}) + \text{I}_2(\text{g}) \rightleftharpoons 2\text{HI}(\text{g}) \]
**Equilibrium Constant:**
The equilibrium constant, \( K \), for this reaction is 0.948 at the temperature of the flask.
**Problem Statement:**
Calculate the equilibrium molarity of hydrogen iodide (HI). Round your answer to two decimal places.
**Input Field:**
\[ \boxed{ \_\_ \text{M} } \]
**Submission Buttons:**
- A checkmark (✔️) for submitting the answer.
- A counterclockwise arrow (
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