Consider the reaction A+B⟶C+D. Is each of the following statements true or false?

1) The rate law for the reaction must be Rate=k[A][B].

2) If the reaction is an elementary reaction, the rate law is second order.

3) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order.

4) The activation energy for the reverse reaction must be greater than that for the forward reaction.

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  • 1 year ago
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    True or False....

    1) The rate law for the reaction must be Rate=k[A][B]..... FALSE. The rate law is determined experimentally, not from the balanced equation unless it is known to be an elementary step.

    2) If the reaction is an elementary reaction, the rate law is second order......TRUE. The reaction is first order in A and in B, and second order overall.

    3) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order...... FALSE. The reverse reaction is Rate = k[C][D] and is second order overall.

    4) The activation energy for the reverse reaction must be greater than that for the forward reaction...... FALSE. There is no way to tell whether the forward reaction (or the reverse reaction) is exothermic or endothermic.

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