The equilibrium constant, Kp. for the following reaction is 55.6 at 698 K:H2(g) +12(8) 2HI(g)Calculate the equilibrium partial pressures of all species when H₂ and I₂, each at an intitial partial pressure of 2.14 atm, areintroduced into an evacuated vessel at 698 K.H₂P12atmatmatmPHI

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Answered: The equilibrium constant, Kp. for the…

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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Enter your answer in the provided box. The equilibrium constant KP for the reaction is 209 at a certain temperature. Calculate PO2 if PNO = 0.671 atm and PNO2 = 0.231 atm. 2NO2(g)⇆ 2NO(g) + O2(g) PO2 = atm
An empty steel container is filled with 0.0580 atm of HF. The system is allowed to reach equilibrium. If Kp = 2.76 for the reaction below, what is the equilibrium partial pressure of H₂? 2 HF (g) ⇌ H₂ (g) + F₂ (g)
At a certain temperature, an equilibrium mixture of O2, SO2, and SO3 contains equal concentrations of of SO2 and SO3. Calculate the concentration of O2 at this temperature if Kc = 19 for the reaction at this temperature. 2 SO2(g) + O2(g) ⇆ 2 SO3(g)
A mixture of 4.1 atm CO2, 2.1 atm H2, and 3.3 atm H₂O are added to a sealed 2.0 L vessel at 500 K and allowed to come to equilibrium according to the reaction below. CO₂(g) + H₂(g) = CO(g) + H₂O(g) Which direction must the reaction proceed based on the initial concentrations? 1. The reaction proceeds forward. 2. The reaction proceeds in reverse. 3. The direction cannot be determined.
The equilibrium reaction between dinitrogen tetraoxide, N2O4(g), and nitrogen dioxide, NO2(g), can be written as the following. N2O4(g) 2 NO2(g) Initially, 0.34 mol N2O4 were introduced into a 0.74 L vessel at 21°C. At equilibrium, 0.24 mol N2O4 were present. What is the value of Kc for this reaction at this temperature?
A mixture of 1.00 Atm of NO, 0.50 Atm of H2, and 1.00 Atm of N2 was allowed to reach equilibrium according to the reaction given below (initially there was no H2O). At equilibrium, the partial pressure of NO was found to be 0.62 Atm. Determine the value of the equilibrium constant, Kp, for the reaction: 2NO(g) + 2H2(g) ⇄ N2(g) + 2H2O(g)
At 1359 °C the equilibrium constant for the reaction: 2 BrCl(g) = Br₂(g) + Cl₂(g) is Kp = 2.11. If the initial pressure of BrCl is 0.00467 atm, what are the equilibrium partial pressures of BrCl, Br₂, and Cl₂? p(BrCl): = p(Br₂) = p(Cl₂): =
Consider the following reaction: A2 (g) + B2 (g) ⇄ 2AB (g) Kp = 25.6 The three species are mixed in a 5.000 L flask and have the following partial pressures: PAB = 0.520 atm, PA₂ = 0.020 atm, PB₂ = 0.450 atm. What is the equilibrium partial pressure of AB in atm? Report your answer with four decimals. Enter numbers only; do not enter units.
The position of equilibrium would not be appreciably affected by changes in the volume of the container for NiO(s) + CO(g) + Ni(s) + CO2(g) BacO3(s) + Ba(s) + CO2(g) O 2H20(g) + 2H2(g) + O2(g) 2C0(g) + O2(g) → 2CO2(g) O PCI5(s) + PCI3(g) + Cl2(g)
At 1000 K, a sample of pure NO₂ gas decomposes: 2 2NO₂(g) = 2NO(g) + O₂(g) The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium. Part 1 of 2 What is the pressure of NO? Be sure your answer has the correct number of significant digits. Part 2 of 2 atm x10 atm X What is the pressure of NO₂? Be sure your answer has the correct number of significant digits. Ś x10
At a given temperature, the system N₂(g) + O₂(g) ≈ 2NO (g) is at equilibrium with Kp = 4.15.The system has the following partial pressures PN 2 1.23 atm and PNO = 5.35 atm. Determine the partial pressure of the oxygen gas present in this equilibrium mixture. -
A student ran the following reaction in the laboratory at 583 K: COCI₂(9) co(g) + Cl₂(9) When he introduced COCI₂(g) at a pressure of 0.417 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of Cl₂(g) to be 0.243 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = =

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