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Chapter 12: Q62 E (page 709)

In terms of collision theory, to which of the following is the rate of a chemical reaction proportional?

(a) the change in free energy per second

(b) the change in temperature per second

(c) the number of collisions per second

(d) the number of product molecules

Short Answer

Expert verified

Option (c)the number of collisions per second

Step by step solution

01

Correct Option

The correct option is (c) the number of collisions per second.

02

Explanation

From the collision state theory, the reaction rate is directly proportional to the number of collisions occurring per second between two reactant molecules.

Therefore option (c) is correct.

The rate of a reaction is independent of the change in free energy per second or the number of product molecules formed

The rate of a reaction is directly proportional to temperature, but there is no dependency on the rate of increase of temperature on the rate of reaction.

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Most popular questions from this chapter

How will each of the following affect the rate of the reaction:

\({\bf{CO}}\left( {\bf{g}} \right){\bf{ + \;N}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {{\bf{O}}_{\bf{2}}}{\bf{\;}}\left( {\bf{g}} \right){\bf{ + NO}}\left( {\bf{g}} \right)\) if the rate law for the reaction is rate = \({\bf{k(NO}}{}_{\bf{2}}{\bf{)(CO)}}\)?

  1. Increasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.1 atm to 0.3 atm
  2. Increasing the concentration of CO from 0.02 M to 0.06 M.

Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces:

\(\begin{aligned}{l}_{{\bf{15}}}^{{\bf{32}}}{\bf{P}} \to _{{\bf{16}}}^{{\bf{32}}}{\bf{S + }}{{\bf{e}}^{\bf{ - }}}\\{\bf{rate = 4}}{\bf{.85 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}\,{\bf{da}}{{\bf{y}}^{{\bf{ - 1}}}}{{\bf{(}}^{{\bf{32}}}}{\bf{p)}}\end{aligned}\)

What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of \({\bf{0}}{\bf{.0033 M}}\)?

Determine which of the two diagrams here (both for the same reaction) involves a catalyst, and identify the activation energy for the catalyzed reaction:

What is the half-life for the decomposition of \({{\bf{O}}_{\bf{3}}}\) when the concentration of \({{\bf{O}}_{\bf{3}}}\)is \({\bf{2}}{\bf{.35 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}\)M? The rate constant for this second-order reaction is 50.4 L/mol/h.

What is the rate equation for the elementary termolecular reaction A + 2B⟶products? For 3A⟶products?
See all solutions

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