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Chemical Kinetics

Question

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For the hypothetical reaction:
$A_{2} + 2 B_{2} \to 2 {AB}_{2},$
write the rate equation in terms of the disappearance of B₂ and formation of AB_2.

Solution

Rate = $- \frac{1}{2} \frac{d [B_{2}]}{dt} = + \frac{1}{2} \frac{d [{AB}_{2}]}{dt}$

Some More Questions From Chemical Kinetics Chapter

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction.

The rate law for the decomposition of N₂O₅ is rate = k[N₂O₅]. What is the significance of k in this equation?

Define activation energy of a reaction.

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