For a gaseous reaction, A2 + 2B 2AB, the following rate data obtained at 250K.Calculate the rate of formation of AB when [A2] = 0.02 M and [B] = 0.01 M at 250K.
Correct answer: B. 4.8 x 10^-6 mole I-l s-l
- A. 4.8 x 10^-5 mole I-l s-l
- B. 4.8 x 10^-6 mole I-l s-l
- C. 5.8 x 10^-6 mole I-l s-l
- D. 5.8 x 10^-5 mole I-l s-l
Explanation
When the concentration of A doubles, the rate of reaction of reaction also doubles. Hence the rate of reaction is first order with respect to A. When concentration of B becomes four times, the rate of reaction also becomes four times. So the rate of reaction is first order with respect to B.Rate = K [A2] [B]
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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