Consider a reaction, $A \to B + C$ . If the initial concentration of A was reduced from 2M to 1M in 1 hour and from 1M to 0.25M in 2 hours, the order of reaction is:

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Solution

The correct option is A 1
The initial concentration of A was reduced from 2M to 1M in 1 hr.
Thus, the concentration is reduced to half and the time is half life period. It is equal to 1 hr.
The concentration of A was reduced from 1M to 0.25M in 2 hours.
Thus, the concentration is reduced to one fourth and the time is two half life periods. It is equal to 2 hrs. Thus, half life is 1 hr.
Hence, the half life is independent of the concentration.
Hence, the reaction is of first order.

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Consider a reaction, A→B+C. If the initial concentration of A was reduced from 2M to 1M in 1 hour and from 1M to 0.25M in 2 hours, the order of reaction is:

Consider a reaction, $A \to B + C$ . If the initial concentration of A was reduced from 2M to 1M in 1 hour and from 1M to 0.25M in 2 hours, the order of reaction is: