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Chemistry Question on Chemical Kinetics

Observe the following reaction ;            A(g)+3B(g)⟶  2C(g)\, \, \, \, \, \, \, \, \, \, \, A(g) + 3B(g) \longrightarrow \, \, 2C(g) The rate of this reaction (−d[A]dt)\big(-\frac{d [A]}{dt}\big) is 3×10−3 mol L−1 min−1.3 \times 10^{-3} \, mol \, L^{-1} \, min^{-1}. What is thd value of −d[B]dt-\frac{d [B]}{dt} in mol L−1 min−1mol \, L^{-1} \, min^{-1}?

A

3×10−33 \times 10^{-3}

B

9×10−39 \times 10^{-3}

C

10−310^{-3}

D

1.5×10−31.5 \times 10^{-3}

Answer

9×10−39 \times 10^{-3}

Explanation

Solution

The rationalised rate =
\hspace20mm -\frac{d [A]}{dt} = -\frac{1}{3} \frac{d [B]}{dt} = \frac{1}{2} \frac{d [C]}{dt}
From this relation we have
\hspace20mm -\frac{d [B]}{dt} = -3 \times \frac{d [A]}{dt}
\hspace33mm = -3 \times 3 \times 10^{-3}
\hspace33mm = 9 \times 10^{-3}