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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
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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POST) question 31.

please answer B and show work thank you 

### 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.
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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