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Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) PC1₂(g) + Cl₂(g) A 0.1924 mol sample of PCI, (g) is injected into an empty 2.10 L reaction vessel held at 250 °C. Calculate the concentrations of PC1, (g) and PCI, (g) at equilibrium. [PCI,] = [PC1₂] = 0.0035 0.08 Incorrect Kc = 1.80 at 250 °C Macmilla M M

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) PC1₂(g) + Cl₂(g) A 0.1924 mol sample of PCI, (g) is injected into an empty 2.10 L reaction vessel held at 250 °C. Calculate the concentrations of PC1, (g) and PCI, (g) at equilibrium. [PCI,] = [PC1₂] = 0.0035 0.08 Incorrect Kc = 1.80 at 250 °C Macmilla M M

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
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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**Phosphorus Pentachloride Decomposition** Phosphorus pentachloride decomposes according to the chemical equation: \[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \] **Equilibrium Constant** \( K_c = 1.80 \) at 250 °C **Problem Statement** A 0.1924 mol sample of \(\text{PCl}_5(g)\) is injected into an empty 2.10 L reaction vessel held at 250 °C. Calculate the concentrations of \(\text{PCl}_5(g)\) and \(\text{PCl}_3(g)\) at equilibrium. **Concentration Calculations:** \[ [\text{PCl}_3] = 0.0035 \, \text{M} \] \[ [\text{PCl}_5] = 0.08 \, \text{M} \] *(This result is marked "Incorrect")*
Transcribed Image Text:**Phosphorus Pentachloride Decomposition** Phosphorus pentachloride decomposes according to the chemical equation: \[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \] **Equilibrium Constant** \( K_c = 1.80 \) at 250 °C **Problem Statement** A 0.1924 mol sample of \(\text{PCl}_5(g)\) is injected into an empty 2.10 L reaction vessel held at 250 °C. Calculate the concentrations of \(\text{PCl}_5(g)\) and \(\text{PCl}_3(g)\) at equilibrium. **Concentration Calculations:** \[ [\text{PCl}_3] = 0.0035 \, \text{M} \] \[ [\text{PCl}_5] = 0.08 \, \text{M} \] *(This result is marked "Incorrect")*
Expert Solution
Step 1

Given reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g)

The initial number of moles of PCl5 = 0.1924 mol

Volume = 2.10 L

We have to calculate the concentrations of PCl5 and PCl3 at equilibrium.

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