For the reaction, 2X3 $$ \rightleftharpoons $$ 3X2, the rate of formation of X2 is
A. $$3\left( {\frac{{ - d\left[ {{X_3}} \right]}}{{dt}}} \right)$$
B. $$\frac{1}{2}\left( {\frac{{ - d\left[ {{X_3}} \right]}}{{dt}}} \right)$$
C. $$\frac{1}{3}\left( {\frac{{ - d\left[ {{X_3}} \right]}}{{dt}}} \right)$$
D. $$\frac{3}{2}\left( {\frac{{ - d\left[ {{X_3}} \right]}}{{dt}}} \right)$$
Answer: Option D
This Question Belongs to Engineering Chemistry >> Chemical Kinetics
Related Questions on Chemical Kinetics
The half-life of a first order reaction varies with temperature according to
A. In t1/2 ∝ 1/T
B. In t1/2 ∝ T
C. t1/2 ∝ 1/T2
D. t1/2 ∝ T2
A. 0.1386 min-1
B. 0.0693 min-1
C. 0.1386 mol L-1min-1
D. 0.0693 mol L-1min-1
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