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NEET CHEMISTRYEasy

If the concentration of a solution is changed from 0.2 to 0.4, then what will be the rate and rate constant? The reaction is of first order and rate constant is k=1×10−6k = 1 \times 10^{-6}:

A

2×10−7 ; 1×10−62 \times 10^{-7} \text{ ; } 1 \times 10^{-6}

B

1×10−7 ; 1×1061 \times 10^{-7} \text{ ; } 1 \times 10^6

C

4×10−7 ; 1×10−64 \times 10^{-7} \text{ ; } 1 \times 10^{-6}

D

2×10−3 ; 1×10−32 \times 10^{-3} \text{ ; } 1 \times 10^{-3}

Step-by-Step Solution

For a first-order reaction, the rate law is given by Rate=k[A]\text{Rate} = k[A]. Substituting the given values, where the rate constant k=1×10−6k = 1 \times 10^{-6} and the new concentration [A]=0.4[A] = 0.4, we get Rate=(1×10−6)×0.4=4×10−7\text{Rate} = (1 \times 10^{-6}) \times 0.4 = 4 \times 10^{-7}. The rate constant of a reaction is independent of the concentration of the reactants (it depends only on temperature and the presence of a catalyst). Therefore, it remains unchanged at 1×10−61 \times 10^{-6}.

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