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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 h

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 h

Chemistry
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 4
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 4
Expert Solution
Step 1

•Here for a given reaction equilibrium constant given which is 3.3

•Initial temperature=> 373 K

•Now some factors are changing and we have to tell their effects on equilibrium constant.

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