D. Complete Me! Use the equation to answer the questions. C6H1206 (s) + 6 O28) → 6 H2O (8) + 6 CO2 (8) 1. What happens to the concentrations of: a. C6H12O6 and O2 as the reaction proceeds >? b. H2O + CO2 as the reaction proceeds →? 2. According to the collision theory, what 3 circumstances are needed for C6H12O6 & O2 to react?

D. Complete Me! Use the equation to answer the questions. C6H1206 (s) + 6 O28) → 6 H2O (8) + 6 CO2 (8) 1. What happens to the concentrations of: a. C6H12O6 and O2 as the reaction proceeds >? b. H2O + CO2 as the reaction proceeds →? 2. According to the collision theory, what 3 circumstances are needed for C6H12O6 & O2 to react?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 8CR

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Similar questions

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. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
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The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?