Part B Initially, 0.65 mol of PC15 is placed in a 1.0 L flask. At equilibrium, there is 0.13 mol of PC13 in the flask. What is the equilibrium concentration of PC15? Express your answer to two significant figures and include the appropriate units. [PC15] = HA Value Units ?
Part B Initially, 0.65 mol of PC15 is placed in a 1.0 L flask. At equilibrium, there is 0.13 mol of PC13 in the flask. What is the equilibrium concentration of PC15? Express your answer to two significant figures and include the appropriate units. [PC15] = HA Value Units ?
Chemistry
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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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![### Consider the Following Reaction:
\[ \text{PCl}_5(g) \leftrightarrow \text{PCl}_3(g) + \text{Cl}_2(g) \]
#### Part A: Equilibrium Constant Expression
Select the correct equilibrium constant expression (Kc) for the reaction:
- \( K_c = \frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \)
- \( K_c = \frac{[\text{PCl}_5]}{[\text{PCl}_3][\text{Cl}_2]} \)
**Correct Choice:**
\[ K_c = \frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \]
**Explanation:**
The product concentrations are in the numerator of the equilibrium-constant expression, and the reactant concentration is in the denominator of the expression. All coefficients in the balanced chemical equation are 1, so there are no exponents in the expression.
#### Part B: Calculate Equilibrium Concentration of \( \text{PCl}_5 \)
Initially, 0.65 mol of \( \text{PCl}_5 \) is placed in a 1.0 L flask. At equilibrium, there is 0.13 mol of \( \text{PCl}_3 \) in the flask. What is the equilibrium concentration of \( \text{PCl}_5 \)?
Express your answer to two significant figures and include the appropriate units.
\[ [\text{PCl}_5] = \text{Value} \, \text{Units} \]
- Input values into the provided box and submit your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F59c9f849-9820-4119-beb6-2f585a7a222b%2F5597eab6-878c-475e-8bfa-c6350dcd8ec0%2Fijabv1_processed.png&w=3840&q=75)
Transcribed Image Text:### Consider the Following Reaction:
\[ \text{PCl}_5(g) \leftrightarrow \text{PCl}_3(g) + \text{Cl}_2(g) \]
#### Part A: Equilibrium Constant Expression
Select the correct equilibrium constant expression (Kc) for the reaction:
- \( K_c = \frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \)
- \( K_c = \frac{[\text{PCl}_5]}{[\text{PCl}_3][\text{Cl}_2]} \)
**Correct Choice:**
\[ K_c = \frac{[\text{PCl}_3][\text{Cl}_2]}{[\text{PCl}_5]} \]
**Explanation:**
The product concentrations are in the numerator of the equilibrium-constant expression, and the reactant concentration is in the denominator of the expression. All coefficients in the balanced chemical equation are 1, so there are no exponents in the expression.
#### Part B: Calculate Equilibrium Concentration of \( \text{PCl}_5 \)
Initially, 0.65 mol of \( \text{PCl}_5 \) is placed in a 1.0 L flask. At equilibrium, there is 0.13 mol of \( \text{PCl}_3 \) in the flask. What is the equilibrium concentration of \( \text{PCl}_5 \)?
Express your answer to two significant figures and include the appropriate units.
\[ [\text{PCl}_5] = \text{Value} \, \text{Units} \]
- Input values into the provided box and submit your answer.
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