Kp only counts with gases molecule , while Kc only counts with aqueous solution+ gases. So here reactant and product both are gaseous that's why only reaction having equal numbers of reactants and products will have kp=kc ie.change in number of moles is equal to 0.option(a) is correct.
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Similar Questions
Q1
The value of KpKc for the following reactions at 300K are, respectively:
N2(g)+O2(g)⇌2NO(g)
N2O4(g)⇌2NO2(g)
N2(g)+3H2(g)⇌2NH3(g) [At300K,RT=24.62dm3atmmol−1]
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Q2
Given: N2(g)+3H2(g)⇌2NH3(g);K1 N2(g)+O2(g)⇌2NO(g),K2 H2(g)+12O2(g)⇌H2O(g);K3
The equilibrium constant for, 2NH3(g)+52O2(g)⇌2NO(g)+3H2O(g)
will be:
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Q3
How many of the following reactions goes almost all the way to completion?N2(g)+O2(g)⇌2NO(g);Kc=2.7×10−18
2NO(g)+O2(g)⇌2NO2(g)
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Q4
List - IList - II(I) Dissociation ofN2O4(g):(P) Increases withN2O4(g)⇌2NO2(g);temperatureΔH=+57.0kJ(II) Oxidation of NH3(g):(Q) Decreases with4NH3(g)+5O2⇌4NO(g)+6H2O(g);pressureΔH=−900.0kJ(III) Oxidation of nitrogen:(R) Increases withN2(g)+O2(g)⇌2NO(g);addition of inertΔH=+180.0kJgas at constantpressure(IV) Formation ofNO2(g):(S) Decreases withNO(g)+O3(g)⇌NO2(g)+O2(g);temperatureΔH=−200.0kJ(T)Kp=Kc(U)Kp=Kc(RT)1
Which of the following options has the correct combination considering List-I and List-II?
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Q5
Consider the following equilibria: (1) N2(g)+3H2(g)⇌2NH3(g) (2) N2(g)+O2(g)⇌2NO(g) (3) PCl5(g)⇌PCl3(g)+Cl2(g) Choose the correct statement(s):