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Chemistry Question on Chemical Kinetics

Consider the reaction, 2A+B→2A + B \to When concentration of BB alone was doubled, the half-life did not change. When the concentration of AA alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is

A

L mol−1 s−1L \,mol^{-1}\, s^{-1}

B

no unit

C

mol−1 s−1mol^{-1}\, s^{-1}

D

s−1s^{-1}

Answer

L mol−1 s−1L \,mol^{-1}\, s^{-1}

Explanation

Solution

2A+B−>Products {2A+B->Pr oducts} When conc. of B is doubled, the half life did not change, hence reaction is of first order w.r.t. B. When concentration of A is doubled, reaction rate is Hence over all order of reaction is 1+1=21 + 1 = 2 So, unit of rate constant mol−1 lit s−1.mol^{-1}\, lit\, s^{-1}. Hence, (1) is correct.