At 1024°C, the pressure of oxygen gas from the decomposition of copper(II)oxide is 0.490 bar: 4 CuO (s) 2 Cu₂0 (s) + O₂(g) a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure) b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C. c. What would the fraction be if a 1.00 mole sample of CuO were used? d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium? e. What is the Gibbs standard energy for this reaction?

At 1024°C, the pressure of oxygen gas from the decomposition of copper(II)oxide is 0.490 bar: 4 CuO (s) 2 Cu₂0 (s) + O₂(g) a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure) b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C. c. What would the fraction be if a 1.00 mole sample of CuO were used? d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium? e. What is the Gibbs standard energy for this reaction?

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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Question

At 1024°C, the pressure of oxygen gas from the decomposition of copper(Il)oxide is 0.490 bar:
4 CuO (s) = 2 Cu2O (s) + O2 (g)
a. What is the value of Kp for this reaction? (Hint: Use 1 atm as your standard pressure)
b. Calculate the fraction of CuO that will decompose if 0.160 mole of it is placed in a 2.00 L flask at 1024°C.
c. What would the fraction be
a 1.00 mole sample of CuO were used?
d. What is the smallest amount of CuO in moles that is needed in order to establish equilibrium?
e. What is the Gibbs standard energy for this reaction?

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