NEET Chemistry Chemical Kinetics Questions Solved


In the following reaction : XA → YB

log[ -d(A)/dt ] = log[-d(B)/dt] +0.3

where -ve sign indicates rate of disappearance the reactant. Then X : Y is

(1) 1:2

(2) 2:1

(3) 3:1

(4) 3:10

(2)  XA → YB

     log[-d(A)/dt ] = log[-d(B)/dt] +0.3

     log[-d(A)/dt ] = log[-d(B)/dt] + log 2

     -da/dt = 2 x -dB/dt

     Hence, X:Y = 2:1

Difficulty Level:

  • 16%
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  • 18%
  • 27%
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