Consider a chemical reaction between two reactants, A and B, that forms a product C. The reaction is exothermic and occurs at a constant temperature. Initially, both reactants are present in equal amounts. However, the reaction rate is found to be significantly faster when reactant A is present in excess compared to when reactant B is present in excess. Explain this observation using principles of reaction kinetics and thermodynamics

Consider a chemical reaction between two reactants, A and B, that forms a product C. The reaction is exothermic and occurs at a constant temperature. Initially, both reactants are present in equal amounts. However, the reaction rate is found to be significantly faster when reactant A is present in excess compared to when reactant B is present in excess. Explain this observation using principles of reaction kinetics and thermodynamics

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 75A

See similar textbooks

Similar questions

Question: Consider a hypothetical chemical reaction A + B → C + D. The reaction is known to be exothermic and highly spontaneous. However, when the reaction is carried out at room temperature, the reaction rate is extremely slow. How can this discrepancy between the thermodynamics and kinetics of the reaction be explained? Provide a detailed explanation.
Question:Consider the following hypothetical scenario: A researcher is investigating the thermodynamics of a chemical reaction. During the course of their experiment, they observe that the reaction does not follow the expected trends according to Le Chatelier's principle. Despite increasing the temperature, the reaction becomes less favorable. They also notice that the reaction rate decreases as the concentration of reactants increases. Explain this unusual behavior and provide a possible explanation.
Question:Consider a hypothetical chemical reaction that involves the conversion of reactants A and B into products C and D. The reaction is known to be highly exothermic and occurs in a closed system at constant temperature and pressure. Based on this information, answer the following question: Why does the rate of reaction decrease over time, even though the reaction is exothermic?
Assuming the net reaction is an exothermic process. Which of the potential energy diagrams best represents the following reaction:
Consider what happens when a sample of the explosive TNT is detonated under atmospheric pressure. (a) Is the detonation a reversible process?
Consider a chemical reaction between compound A and compound B. The reaction proceeds via a multi-step mechanism involving several intermediates and transition states. The overall reaction is exothermic, but one of the intermediate steps is endothermic. Explain how the endothermic intermediate step can still be consistent with the overall exothermic nature of the reaction.
A two-step reaction is spontaneous in the forward direction. The second step of the reaction is rate determining. Draw a graph of energy vs. reaction coordinate for the reaction. Label the activation of each forward step and the transition states of each step.
If heat is given to an endothermic reaction, the reaction will ________ not shift at all because equilibrium is independent of reaction rate not shift at all because equilibrium is independent of temperature shift towards the reactants shift towards the products
Which would you predict to react at a faster rate when all other conditions are equal? Br2 gas Br2 liquid
Using your knowledge of temperature and reaction rate, explain why food spoils at a slower rate when refrigerated.
Describe how chemical reactions are affected by reaction conditions.- What is measured by the heat of the reaction?- What is meant by the rate of a chemical reaction?
is chemical reactions and reaction rate the same?