TASK 3: COMPLETE THE TABLE! Does this increase or Explain why using Collision Theory. Change in condition: decrease the rate of reaction? Ex: Increases (speeds up) Ex: Molecules move faster & collide more = Increased reaction rate a. Increasing the temperature b. Increasing the concentration of CSH12O6 c. Decreasing the concentration of O2 d. Increase the surface area by chewing up food in your mouth e. Decreasing the temperature f. Increasing the pressure in the container g. Decreasing the concentration of H2O h. Increasing the volume container the reaction occurs in i. Increasing the concentration of CO2 j. Using a catalyst (like salivary amylase)

TASK 3: COMPLETE THE TABLE! Does this increase or Explain why using Collision Theory. Change in condition: decrease the rate of reaction? Ex: Increases (speeds up) Ex: Molecules move faster & collide more = Increased reaction rate a. Increasing the temperature b. Increasing the concentration of CSH12O6 c. Decreasing the concentration of O2 d. Increase the surface area by chewing up food in your mouth e. Decreasing the temperature f. Increasing the pressure in the container g. Decreasing the concentration of H2O h. Increasing the volume container the reaction occurs in i. Increasing the concentration of CO2 j. Using a catalyst (like salivary amylase)

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 9CR

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Similar questions

use the kineticmolecular theory to explain why an increase in temperature increases reaction rate.
Characterize a system at chemical equilibrium with respect to each of the following a. the rates of the forward and reverse reactions b. the overall composition of the reaction mixture For a general reaction3A(g)+B(g)2C(g), if one starts an experiment with only reactants present, show what the plot of concentrations of A, B, and C versus time would look like. Also sketch the plot illustrating the rate of the forward reaction and rate of the reverse reaction versus time.
Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.
Consider the following activation energy diagram. Which of the following statements about the diagram are true? (a) E a(forward)E a(reverse)(b) B represents the activation energy of the forward reaction. (c) Energy (H)for the reaction is AC. (d) E a(forward)=BA(e) E a(forward)=E a(reverse)C
How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.
. Account for the increase in reaction rate brought about by a catalyst.
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
In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.