### Equilibrium Constant for Gas-Phase Thermal DecompositionA mixture of isobutylene \((\text{(CH}_3)_2\text{CCH}_2, 0.400 \,\text{bar partial pressure})\) and HCl \((0.600 \,\text{bar partial pressure})\) is heated to \(500.0 \,\text{K}\). The equilibrium constant \(K\) for the gas-phase thermal decomposition of tert-butyl chloride \((\text{(CH}_3)_3\text{CCl})\) is \(3.45\) at \(500.0 \,\text{K}\).\[(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}\]Based on your ICE table, set up the expression for \(K\) for the decomposition of \((\text{CH}_3)_3\text{CCl}\).\[(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}\]**Graphical Representation:**The image contains a horizontal equilibrium bar showing the balance between the reactants and products. The bar is divided into a dark segment and a light segment, each representing different parts of the equilibrium reaction.**Expression for the Equilibrium Constant \(K\):**\[K = \frac{\text{[Products]}}{\text{[Reactants]}} = 3.45\]*Note: Do not combine or simplify terms.*### Key Facts:- **Initial Conditions:** - Isobutylene: 0.400 bar - HCl: 0.600 bar- **Temperature:** - Heated at 500.0 K- **Equilibrium Reaction:** \[ (\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)} \]Ensure that the expression derived from your

The equilibrium constant for a gaseous phase reaction is expressed in terms of the ratio of the…

A mixture of isobutylene ((CH:)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH:):CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) %3D Based on your ICE table, set up the expression for K for the decomposition of (CH:):CCI. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) 1 Do not combine or simplify terms. K = 3.45 %3D

A mixture of isobutylene ((CH:)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH:):CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) %3D Based on your ICE table, set up the expression for K for the decomposition of (CH:):CCI. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) 1 Do not combine or simplify terms. K = 3.45 %3D

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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At high temperature, HCl and O2 react to give Cl2 gas: 4HClg) + O2(g) ⇌ 2 Cl2 (g) + 2H2O(g) If HCl at 2.30 bar and O2 at 1.00 bar react at 750K, the equilibrium pressure of Cl2 is measured to be 0.93 bar. Determine the value of Keq at 750 K. Use a systematic approach to include setting up an ICE table, constructing equilibrium constant expression and show calculation involved.
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Given the reaction: CO(NH2),(s) + H2O(g) = CO2(9) + 2NH3(g) -- Kp If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be = 1.39 at 500 K The value of K, for the given reaction at 600 K is The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is -- A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase. This means that:
At 500 K, the Kp of the reaction PCl5 (g) = PCl3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we mix the gases, and their partial pressures are given by P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Which of the following statements is/are correct regarding how the mixture will proceed to reach equilibrium? a) The partial pressure of PCl3 will increase during the reaction course to reach equilibrium. b) The partial pressure of PCl5 will increase during the reaction course to reach equilibrium. c) The reaction Gibbs energy change ∆G is less than zero for the above condition: P (PCl5(g)) = 0.325 atm, P(PCl3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Note that the question is about ∆G not ∆Go. a) only b) only c) only a) and b) b) and c) a) and c) a), b) and c) None of the 3 statements is correct.
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The Kp for th reaction 2 A2B(g)⇌ 2 A(g)+B2 (g) is 2.2*10^-5. The gas is introduced to the reaction vessel of a fixed volume at the partial pressure of 0.010 atm. Explain how you would find the total pressure at equilibrium. The systems temperature is the same for the Kp value and stays constant for the entire reaction. You do not have to solve for the actual pressure, but explain what would be used to do so.
At 500 K, the Kp of the reaction PCI5 (g) = PCI3 (g) + Cl2 (g) is 0.497. In a chamber at 500 K, we mix the gases, and their partial pressures are given by P (PCI5(g)) = 0.325 atm, P(PCI3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 atm. Which of the following statements is/are correct regarding how the mixture will proceed to reach equilibrium? a) The partial pressure of PCI3 will increase during the reaction course to reach equilibrium. b) The partial pressure of PCI5 will increase during the reaction course to reach equilibrium. c) The reaction Gibbs energy change AG is less than zero for the above condition: P (PCI5(g)) = 0.325 atm, P(PCI3 (g)) = 0.132 atm and P(Cl2(g)) = 0.241 %3D %3D atm. Note that the question is about AG not AGº.
NOBr(g) at 1 bar pressure is introduced into a evacuated chamber according to the equilibrium equation give below, it dissociates; 2NOBr(g) <=> 2NO(g) + Br2(g) at 25 degrees Celsius equilibrium is reached, the partial pressure is 0.60 bar of the NOBr. At 25 degrees Celsius what is the equilibrium constant for this reaction. Chose the most correct answer. a) 0.012 b) 0.062 c) 0.089 d)1.34
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