The reaction N2O4−⇀↽−2NO2 is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.327 mol/L N2O4 and 1.91 mol/L NO2 . Calculate the equilibrium constant, Kc , for this reaction. Kc= 11.16     An additional 1.00 mol NO2 is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. towards the product towards the reactant no change Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc . Kc will increase Kc will not change Kc will decrease Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N2O4]=   mol/L [NO2]=   mol/L

Question

The reaction

N2O4−⇀↽−2NO2

is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.327 mol/L N2O4 and 1.91 mol/L NO2 .

Calculate the equilibrium constant, Kc , for this reaction.

Kc= 11.16
 
 
An additional 1.00 mol NO2 is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added.
towards the product
towards the reactant
no change
Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc .
Kc will increase
Kc will not change
Kc will decrease
Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution.
[N2O4]=
 
mol/L
[NO2]=
 
mol/L
 

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