Hydrogen flouride decomposes into hydrogen and fluorine gas. The value of K at room temperature is 1.0 x 10-95. From the value of the equilibrium constant do you think the decomposion occurs to any great extent at room temperature? If an equilibrium mixture at room temperature in a 1.0 liter vessel contains 1.0 mol of HF, what is the concentration of H2? Does this result agree with your prediction about the decomposition?
Hydrogen flouride decomposes into hydrogen and fluorine gas. The value of K at room temperature is 1.0 x 10-95. From the value of the equilibrium constant do you think the decomposion occurs to any great extent at room temperature? If an equilibrium mixture at room temperature in a 1.0 liter vessel contains 1.0 mol of HF, what is the concentration of H2? Does this result agree with your prediction about the decomposition?
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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Hydrogen flouride decomposes into hydrogen and fluorine gas. The value of K at room temperature is 1.0 x 10-95. From the value of the equilibrium constant do you think the decomposion occurs to any great extent at room temperature? If an equilibrium mixture at room temperature in a 1.0 liter vessel contains 1.0 mol of HF, what is the concentration of H2? Does this result agree with your prediction about the decomposition?
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