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AP®︎/College Chemistry

Course: AP®︎/College Chemistry > Unit 5

Lesson 1: Reaction rates

Reaction rates

AP.Chem: TRA‑3 (EU), TRA‑3.A (LO), TRA‑3.A.1 (EK), TRA‑3.A.2 (EK), TRA‑3.A.3 (EK)

\ce{Mg}(s) + \ce{2HCl}(aq) \rightarrow \ce{MgCl2}(aq) + \ce{H2}(g)

The reaction between M, g, left parenthesis, s, right parenthesis and H, C, l, left parenthesis, a, q, right parenthesis is represented by the equation above. In a kinetics experiment, a 0, point, 080, space, g sample of M, g, left parenthesis, s, right parenthesis ribbon is added to an Erlenmeyer flask containing 50, space, m, L of 3, point, 0, M, H, C, l, left parenthesis, a, q, right parenthesis at 25, degree, start text, C, end text. The rate of the reaction is determined by measuring the volume of

\ce{H2}(g)

produced every five seconds.

Which of the following experimental changes is most likely to decrease the rate of $\ce{H2}(g)$ production?

(Choice A)
Using a 0, point, 080, space, g sample of powdered M, g, left parenthesis, s, right parenthesis instead of M, g, left parenthesis, s, right parenthesis ribbon
(Choice B)
Using 25, space, m, L of 3, point, 0, M, H, C, l, left parenthesis, a, q, right parenthesis solution instead of 50, space, m, L
(Choice C)
Using a 1, point, 5, M solution of H, C, l, left parenthesis, a, q, right parenthesis instead of a 3, point, 0, M solution
(Choice D)
Heating the H, C, l, left parenthesis, a, q, right parenthesis solution to 30, degree, start text, C, end text before adding the M, g, left parenthesis, s, right parenthesis

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AP®︎/College Chemistry

Course: AP®︎/College Chemistry > Unit 5

Problem