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Indicate whether each statement is true or false.
(a) If you compare two reactions with similar collision factors, the one with the larger activation energy will be faster.
(b) A reaction that has a small rate constant must have a small frequency factor.
(c) Increasing the reaction temperature increases the fraction of successful collisions between reactants.

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Reid Wolff
Reid WolffLv2
28 May 2020

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Related questions


Chemical reactions occur when molecules or atoms collide, the bondsbetween atoms are broken, and new bonds are formed. Breaking thebonds of the reactants requires energy; bond formation releasesenergy. Which of the following statements regarding energy changesduring a reaction are true?
(A)The activation energy (Ea) of the forward reaction is thedifference between the energy of the products and the energy of thetransition state.
(B)If the heat of reaction, ?H, is positive, the energy of theproducts is lower than the energy of the reactants, and thereaction is endothermic.
(C)When the activation energy is low, the reaction rate isslow.
(D)Two or more atoms must collide, with proper orientation, withenergy greater than or equal to the activation energy for areaction to occur.
(E)Increasing the concentration of reactants increases the numberof collisions, and the reaction goes faster.
(F)The energy of a collision between atoms or molecules must begreater than the activation energy (Ea) for bonds to bebroken.
(G)Decreasing the temperature decreases the kinetic energy of thereactants, and the reaction goes more slowly.

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