0.4 mol of X is placed in an empty 1.00 L flask and the temperature is raised to 290°C. The following reaction takes place: 2 X (g) Y (g) + Z (g) At equilibrium, the [Y] = 0.10 M. Determine the equilibrium constant, K, at 290°C. Enter your answer to 3 significant figures and enter a number in scientific notation enter 1 x 10-³ as 1E-3)
0.4 mol of X is placed in an empty 1.00 L flask and the temperature is raised to 290°C. The following reaction takes place: 2 X (g) Y (g) + Z (g) At equilibrium, the [Y] = 0.10 M. Determine the equilibrium constant, K, at 290°C. Enter your answer to 3 significant figures and enter a number in scientific notation enter 1 x 10-³ as 1E-3)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.40QE
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Please my heart hand written not allowed.
![0.4 mol of X is placed in an empty 1.00 L flask and the temperature is raised to 290°C. The following reaction takes place:
2 X (g) - Y (g) + Z (g)
At equilibrium, the [Y] = 0.10 M. Determine the equilibrium constant, K, at 290°C.
Enter your answer to 3 significant figures and enter a number in scientific notation enter 1 x 10-³ as 1E-3)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faa86593d-f70a-45b0-b625-c80fadb8b525%2Fea1aaf5a-ec55-42b8-a0e6-feb74f226014%2Fp6gwzve_processed.jpeg&w=3840&q=75)
Transcribed Image Text:0.4 mol of X is placed in an empty 1.00 L flask and the temperature is raised to 290°C. The following reaction takes place:
2 X (g) - Y (g) + Z (g)
At equilibrium, the [Y] = 0.10 M. Determine the equilibrium constant, K, at 290°C.
Enter your answer to 3 significant figures and enter a number in scientific notation enter 1 x 10-³ as 1E-3)
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