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?
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 51QAP: . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular...
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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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