Reaction mechanisms and the rate-determining step

Evaluate a proposed mechanism by checking that its elementary steps add up to the overall equation and that the slow step matches the rate equation, and distinguish intermediates (formed then consumed) from transition states on energy profiles.

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(i) State the products of the overall reaction. (ii) Sketch the energy profile for this reaction on the axes below. Label the reactants, the products, the transition states and the intermediate. (iii) Deduce the rate equation for the overall reaction.

Which species is an intermediate in the following reaction mechanism? $\ce{NO2(g) + NO2(g) -> NO3(g) + NO(g)}$ $\ce{NO3(g) + CO(g) -> NO2(g) + CO2(g)}$ A. $\ce{NO2}$ B. $\ce{NO3}$ C. $\ce{NO}$ D. $\ce{CO2}$

The following mechanism has been proposed for the reaction between nitrogen(II) oxide and hydrogen. $\ce{2NO(g) <=> N2O2(g)}$ fast $\ce{N2O2(g) + H2(g) -> N2O(g) + H2O(g)}$ slow Which rate equation is consistent with this mechanism? A.…

The energy profile of a reaction that occurs in two steps is shown. Which statement is correct? A. Q is a transition state, and the first step is rate-determining. B. Q is an intermediate, and the first step is rate-determining. C. Q is an intermediate, and…

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