21. At 25°C, Kp = 2.9 x 10³ for the following balanced chemical reaction: A (s) 2 B (g) + C (g) A (s) is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium. Assume at equilibrium that some solid A remains in the container. A) 0.89 atm B) 0.27 atm C) 1.3 atm D) 1.8 atm

21. At 25°C, Kp = 2.9 x 10³ for the following balanced chemical reaction: A (s) 2 B (g) + C (g) A (s) is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium. Assume at equilibrium that some solid A remains in the container. A) 0.89 atm B) 0.27 atm C) 1.3 atm D) 1.8 atm

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

The equilibrium constant Kp for the reaction CCl4(g) —> C(s) + 2Cl2(g) at 700˚C is 0.76. Determine the initial pressure of carbon tetrachloride that will produce an equilibrium pressure of 1.5 atm for Cl2 at 700˚C. (Since C is a solid it can be left out of the ICE chart.)
EXPLAIN STEP BY STEP
A pure sample of SO3 is placed in a container and reacts according to the equation 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 4.00At equilibrium the partial pressure of O2 is 0.10 atm. Calculate the pressure of SO3 remaining at equilibrium.
10) For the reaction: 2 V PC13(g) + Cl2(g) → PC15(g) at 85°C, Kp = 1.19 = If one starts with 2.00 atm pressure of PC13, 1.00 atm pressure of Cl2 and no PC15, what is the partial pressure of PC15(g) at equilibrium? A) 0.739 atm B) 0.621 atm C) 0.465 atm D) 0.167 atm E) 0.553 atm
Hydrogen iodide can decompose into hydrogen and iodine gases. 2 HI(g) --> H2(g) + I2(g) Kp = 0.0180 If 0.05 atm is sealed in flask initially, what is the partial pressure of I2(g) at equilibrium?
At a given temperature, an equilibrium mixture associated with the reaction A(g) + 2 B(g) = 2 C(g) contains: [A] = 0.0250 M [B] = 0.150 M [C] = 0.550 M What is the value of K, for this reaction at the same temperature?
Br2(g) + Cl2(g)  2BrCl(g)If the partial pressures in an equilibrium mixture of Br2, Cl2, and BrCl are 1.12 atm, 1.26 atm, and 3.14 atm, respectively, Find Kp for this reaction at this temperature.
The reaction H2(g) + I2(g)  2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.01 atm and H2 at a pressure of 2.62 atm. Calculate the equilibrium pressure of I2(g) in this mixture.
At 1560 oC the equilibrium constant for the reaction: 2 IBr(g)  I2(g) + Br2(g) is KP = 0.846. If the initial pressure of IBr is 0.00674 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?p(IBr) =  p(I2) =  p(Br2) =
An empty steel container is filled with 0.840 atm of A and 0.840 atm of B. The system is allowed to reach equilibrium according to the reaction below. If Kp = 340 for this reaction, what is the equilibrium partial pressure of C? A (g) + B (g) = C (g)
At 1000 K, the partial pressures of the gases in an equilibrium mixture are 0.71 atm CH4, 1.41 atm H20, 1.00 atm CO, and 3.00 atm H2. What is the value of Kp for the reaction at 1000 K?
The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15