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Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M

Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 76AP: Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the...
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Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M
Transcribed Image Text:Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M
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