### Equilibrium Constants and ICE Tables in Chemical Reactions**Introduction to the Problem:**A mixture of isobutylene \(((CH_3)_2CCH_2\), 0.400 bar partial pressure) and HCl (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 \(((CH_3)_3CCl)\) is 3.45 at 500.0 K.The reaction is as follows:\[(CH_3)_3CCl(g) \leftrightharpoons (CH_3)_2CCH_2(g) + HCl(g)\]**Objective:**Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine the partial pressures of all reactants and products.**ICE Table:**| | \((CH_3)_3CCl(g)\) | \(\leftrightharpoons\) | \((CH_3)_2CCH_2(g)\) | + | \(HCl(g)\) ||--------------------------|--------------------|------------------------|----------------------|------------|---------------|| **Initial (bar)** | | | | | || **Change (bar)** | | | | | || **Equilibrium (bar)** | | | | | |**Instructions for ICE Table Completion:**1. **Identify Initial Pressures:** - **(CH_3)_3CCl(g):** (To be determined) - **(CH_3)_2CCH_2(g):** 0.400 bar - **HCl(g):** 0.600 bar2. **Determine Changes in Pressures:** Use \( x \) to represent the change. - **(CH_3)_3CCl(g):** -x - **(CH_3)_2CCH_2(g):** +x - **HCl(g):** +x3. **Calculate Equilibrium Pressures:** - **(CH_3)_3CCl(g):** Initial - x - **(CH_3)_2CCH_2(g):** \( 0.

Answered: Image /qna-images/answer/168dd0de-ca89-44d9-abe3-552e2c100ffc.jpg

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:):CCH2(g) + HCI(g) Based on the given values, fill in the ICE table to determine the partial pressures of all| reactants and products. 1 Complete the ICE table below. (CH:).CCI(g) (CH:):CCH:(g) HCI(g) Initial (bar) Change (bar) Equilibrium (bar) 5 RESET 1 0.400 0.600 0.200 +x -X Activate W -2х 2x 0.600 - x 0.400 - x 0.600 + x 0.400 + x 0.200 + x 0.200 - x Go to Settings 3.45

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:):CCH2(g) + HCI(g) Based on the given values, fill in the ICE table to determine the partial pressures of all| reactants and products. 1 Complete the ICE table below. (CH:).CCI(g) (CH:):CCH:(g) HCI(g) Initial (bar) Change (bar) Equilibrium (bar) 5 RESET 1 0.400 0.600 0.200 +x -X Activate W -2х 2x 0.600 - x 0.400 - x 0.600 + x 0.400 + x 0.200 + x 0.200 - x Go to Settings 3.45

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...

See similar textbooks

Similar questions

Consider the following reaction: 2H2O(g) + 2SO2(g) ⇌ 2H2S(g) + 3O2(g) A reaction mixture initially contains 6.2 bar H2O and 4.8 bar SO2. Determine the equilibrium partial pressure of H2S if K for the reaction at this temperature is 1.3 × 10-6 Please explain with full calculations
A reaction vessel at 408.5 K contains a mixture of Cl(g) (P = 3.060 bar) and SO2(g) (P = 1.258 bar). The following reaction occurs: Part A Cl2(g) + SO2(g) SO2CI2(g) Determine the equilibrium constant, K. At equilibrium the total pressure is 3.126 bar.
Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .
dont provide hnadwritng solution....
Please don't provide handwritten solution ....
2NaHCO3(s)<--> Na2CO3(s) + H2O(g) + CO2(g), KP(300 °C) = 1.55 atm2, H°rxn = +136 kJ1) When a sample of NaHCO3(s) alone is heated in a sealed volume at 300 °C, it comes to equilibrium with KP(300 °C) = 1.55 atm2, Peq(CO2) = _____ atm, Peq(H2O) = _____ atm,and the total P = _____ atm.
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
In the gas-phase reaction A + B=C+ 2 D, it was found that, when 2.00 mol A, 1.00 mol B and 3.00 mol D were mixed and allowed to come to equilibrium at 25°C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate Kp. [.960]
Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375 X (b) What is Kp if the total pressure is 10.5 atm? 9.12
Keq for a Gas-Phase Reaction A 5.00-L vessel contained 9.49×102 mol of gaseous PCI3, 8.03×102 mol of gaseous PCI5, and 8.21x102 mol of Cl2 gas at equilibrium at 233°C. Calculate the value of Keg (expressed in terms of the molar concentrations) for the reaction PCI3(g) + Cl2(g) = PCI5(g) (No units required.)
2
12.48 The following reaction is in equilibrium in lake water: HCO3(aq) + H+ (aq) = H₂CO3(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. (a) NaHCO3 is added to the lake. (b) H₂CO3 is added. (c) NaOH is added.