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1 mole of NO2 and 2 moles of CO are enclosed in a one litre vessel to attain the following equilibrium NO2 + CO NO + CO2 . It was estimated that at equilibrium , 25 % of initial amount of CO is consumed . The equilibrium constant Kp is--- (1) 1(2) 1/4(3) 1/2(4) 1/3

Since 1 mole of NO2 reacts with 1 mole of CO ,Thus 25% of CO i.e 1/2 moles out of 2 moles have reacted with 1/2 moles of NO2
                       
Initial amount 1             2                   0             0                  
at equilibrium 1/2 3/2 1/2 1/2
         


Kc=[(1/2)(1/2)]/[(1/2)(3/2)] =1/3

Kp=Kc(RT)Δn

Δn = change in no. of moles =no. of moles of product- no. of moles of reactant
Δn = (1+1)-(1+1)=0

thus 
Kp =Kc =1/3
 

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The reaction 2 NO (g) + O2 (g) 2 NO2 (g) has KC = 100.0 at a certain temperature. What is the value for KC for the reaction 2 NO2 (g) 2 NO (g) + O2 (g)? 19. The equilibrium constants at some temperature are given for the following reactions: 2 NO (g) + O2 (g) 2 NO2 (g) KC = 1.4 NO (g) + Br2 (g) NOBr (g) Using this information, determine the value of the equilibrium constant for the following reaction at the same temperature. N2 (g) + O2 (g) + Br2 (g) NOBr (g) 20. Indicate whether the following statement is true or false and explain your reasoning. The value of KC for the reaction 2 AB (g) + Br2 (g) 2 AB2 (g) must be less than the value of KC for the reaction 2 AB2 (g) 2 AB (g) + Br2 (g

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