In this chapter we have seen a number of reactions in which a single reactant fo

Question

In this chapter we have seen a number of reactions in which a single reactant forms products. For example, consider the following first-order reaction: CH3NC(g) to CH3CN(g) However, we also learned that gas-phase reactions occur through collisions.

a possible mechanism involves one step in which two CH3NC molecules collide, resulting in the activation of one of them. In a second step the activated molecule goes on to form the product. Write down the mechanism and determine what step must be rate determining in order for the kinetics of the reaction to be first order. SHow explicitly how the mechanism predicts first order kinetics.

Explanation / Answer

If 2 molecules of (CH3)2NC coolide with each other in a single

elementary step

CH3NC(g) + CH3NC(g) => 2 CH3CN(g)

Rate = k[CH3NC]^2 = k[CH3NC]2

=> reaction is second order (order = 2)

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