Interpretation:Thereason of increase in rate of reaction in the presence of catalyst with the difference between homogenous and heterogeneous catalyst needs to be explained. Whether the reaction has a same or different rate law for both catalyzed and an un-catalyzed pathway needs to be explained.
Concept Introduction:
For a chemical reaction to occur, two most important requirements are activation energy to reactant molecule and correct orientation of reactant molecules to colloid and form product.
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Chapter 15 Solutions
Chemical Principles
- Why does a catalyst increase the rate of a reaction? What is the difference between a homogeneous catalyst and a heterogeneous catalyst? Would a given reaction necessarily have the same rate law for both a catalyzed and an uncatalyzed pathway? Explain.arrow_forward. find the rate law predicted for a particular reaction mechanism.arrow_forwardIf a reaction has the same rate constant, what time does it take for a reactant to decrease by 5 that is, still near the beginning of the reaction process if the kinetics are zeroth-order, first-order, and second-order with respect to that reactant?arrow_forward
- Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.arrow_forwardExplain how a species might be part of a rate law but not part of a balanced chemical reaction.arrow_forward
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