In the gas phase, NO and NO2 react according to NO(g) + NO2 (g) W N2O3 (g) An ev

Question

In the gas phase, NO and NO2 react according to

NO(g) + NO2 (g) W N2O3 (g)

An evacuated flask at 298 K is filled to a pressure of 0.60 bar with N2O3 (g). After equilibrium is established, the partial pressure of NO2 (g) is 0.48 bar.

a) Determine KP for this reaction.

b) Briefly explain what will happen if a catalyst is added after the reaction has reached equilibrium.

c) What will happen if the temperature is increased after the reaction has reached equilibrium? Briefly explain how you arrived at your answer.

Explanation / Answer

The reaction:

NO + NO2 = N2O3

P-N2O3 = 0.6 bar

P-NO = 0

P-NO2 = 0

in equilibrium

P-N2O3 = 0.6 + x

P-NO = 0 - x

P-NO2 = 0 - x

Clearly, x should be negative

we know that

P-NO2 = 0 - x = 0.48

so

x = -0.48

substitute

P-N2O3 = 0.6 + x = 0.60-0.48 = 0.12

P-NO = 0 - x = --0.48 = 0.48

P-NO2 = 0 - x = --0.48 = 0.48

For Kp

KP =P-N2O3 /(P-NO*P-NO2)

Kp = (0.12)/(0.48 *0.48 ) = 0.520833

b)

if we add a catalyst, the equilibrium will be achieved FASTER, but in the same ratios, i.e. the Kp is constant, so partial pressures will be constant as well

c)

If we increase T, and keep Volume of container constant, Pressure will inecrease

this favours the least mol of gases formatino, whichi is N2O3, the shift goes from reactants to products

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