For a first order reaction- A-Product- the rate of reaction at -A-0-2 mol L-1 is 1-0- 10-2 mol L-1 min-1- The half-life period for the reaction is-

The rate of a first-order reaction is $0.04 m o l^{- 1} s^{- 1}$ at 10 seconds and 0.03 $m o l^{- 1} s^{- 1}$ at 20 seconds after initiation of the reaction. The half-life period of the reaction is

Q. The rate for a first order reaction is

0.639 \times 10^{- 2} m o l d m^{- 1} m i n^{- 1}

and the initial concentration is 0.2 mol

d m^{- 3}

. The half-life period is

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For a first order reaction, A→Product, the rate of reaction at [A]=0.2 mol L−1 is 1.0×10−2 mol L−1 min−1. The half-life period for the reaction is:

The correct option is A 832 sLet us considwer the problem:-r=[A]Implies that k=10−20.2=5.0×10−2Therefore t12=0.693KPutting value of k in above equation, we have t12=0.6935.0×10−2=13.86 minHance,=832 sec

For a first order reaction, $A \to$ Product, the rate of reaction at $[A] = 0.2$ mol $L^{- 1}$ is $1.0 \times 10^{- 2}$ mol $L^{- 1}$ $m i n^{- 1}$ . The half-life period for the reaction is: