Consider a reaction X + Y → Products. If the initial concentration of X is increased to four times of its original value, keeping the concentration of Y constant, the rate of reaction increases four-fold. When the concentration of both X and Y becomes four times their original values, the rate of reaction becomes 16 times its original value. The observed rate law is

Question

Consider a reaction X + Y → Products. If the initial concentration of X is increased to four times of its original value, keeping the concentration of Y constant, the rate of reaction increases four-fold. When the concentration of both X and Y becomes four times their original values, the rate of reaction becomes 16 times its original value. The observed rate law is, k [ X ] 2 [ Y ] 2, k [ X ] 1 [ Y ] 2, k [ X ] 1 [ Y ] 1, k [ X ] 2 [ Y ] 1

MARKS App · Accepted Answer

r 1 = k [ X ] m [ Y ] n …(i) r 2 = 4 r 1 = k [ 4 X ] m [ Y ] n …(ii) r 3 = 16 r 1 = k [ 4 X ] m [ 4 Y ] n …(iii) Divide equation (ii) by equation (i) 4 = ( 4 ) m ( 4 ) 1 = ( 4 ) m m = 1 Divide equation (iii) by equation (ii), 4 = ( 4 ) n ( 4 ) 1 = ( 4 ) n n = 1 . Hence rate = k [ X ] 1 [ Y ] 1

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