Equilibrium - Result Question 8

####9. The reaction 2A(g)+B(g)3C(g)+D(g) is begun with the concentrations of A and B both at an initial value of 1.00M. When equilibrium is reached, the concentration of D is measured and found to be 0.25M. The value for the equilibrium constant for this reaction is given by the expression

[2010]

(a) [(0.75)3(0.25)]÷[(0.75)2(0.25)]

(b) [(0.75)3(0.25)]÷[(1.00)2(1.00)]

(c) [(0.75)3(0.25)]÷[(0.50)2(0.75)]

(d) [(0.75)3(0.25)]÷[(0.50)2(0.25)]

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Solution:

  1. (c)

Mole ratio

2A(g)+B(g)3C(g)+D(g)

 Molar concentration 1100 at t=0

 Molar 0.500.750.750.25

concentration at equilibrium

Kc=[C]3[D][A]2[B]=(0.75)3(0.25)(0.50)2(0.75)



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