1.

The reaction X to Product, follows first order kinetics . In 40 minutes the concentration of X changes from 0.1 to 0.025 M . The rate of reaction , when concentration of X is 0.01 M is

Answer»

`1.73 XX 10^(-4) M "min"^(-1)`
`3.47 xx 10^(-5) M "min"^(-1)`
`3.47 xx 10^(-4) M "min"^(-1)`
`1.73 xx 10^(-5) M "min"^(-1)`

Solution :Since 0.1 M of X changes to `0.025` M in 40 minutes , `t_(1//2)` of REACTION = 40/2 = 20 minutes
Rate of reaction of
X = k[X] = `(0.693)/(t_(1//2)) xx [X] = (0.693)/(20) xx 0.01 = 3.47 xx 10^(-4) M "min"^(-1)`.


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