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Chemistry Question on Chemical Kinetics

Observe the following reaction : A(g)+3B(g)→2C(g)A(g)+3B(g)\xrightarrow{{}}2C(g) The rate of this reaction (−d[A]dt)\left( -\frac{d[A]}{dt} \right) is 3×10−3 mol L−1.3\times {{10}^{-3}}\,\text{mol}\,{{\text{L}}^{-1}}. What is the value of −d[B]dt-\frac{d[B]}{dt} in mol L−1min⁡−1.\text{mol}\,{{\text{L}}^{-1}}{{\min }^{-1}}. ?

A

3×10−33\times {{10}^{-3}}

B

9×10−39\times {{10}^{-3}}

C

10−3{{10}^{-3}}

D

1.5×10−31.5\times {{10}^{-3}}

Answer

9×10−39\times {{10}^{-3}}

Explanation

Solution

The rationalised rate = −d[A]dt=−13d[B]dt=12d[C]dt\frac{-d[A]}{dt}=-\frac{1}{3}\frac{d[B]}{dt}=\frac{1}{2}\frac{d[C]}{dt} From this relation we have −d[B]dt=−3×d[A]dt\frac{-d[B]}{dt}=-3\times \frac{d[A]}{dt} =−3×3×10−3=9×10−3=-3\times 3\times {{10}^{-3}}=9\times {{10}^{-3}}