Two mechanisms are proposed for the reaction
Mechanism 2:
Show that each of these mechanisms is consistent with the observed rate law:
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Chemistry: Principles and Reactions
- The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?arrow_forwardClassify 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.arrow_forwardAmmonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)NH4+(aq)+OH(aq) Will any of the following increase the percent of ammonia that is converted to the ammonium ion in water? (a) Addition of NaOH (b) Addition of HCI (c) Addition of NH4CIarrow_forward
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- An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.arrow_forward. Suppose K=4.5103at a certain temperature for the reaction PCl5(g)PCl3(g)+Cl2(g)If it is found that the concentration of PCl5is twice the concentration of PCl3, what must be the concentration of Cl2under these conditions?arrow_forward. In your own words, paraphrase Le Châtelier’s principle. Give an example (including a balanced chemical equation) of how each of the following changes can affect the position of equilibrium in favor of additional products for a system: the concentration of one of the reactants is increased: one of the products is selectively removed from the system: the reaction system is compressed to a smaller volume: the temperature is increased for an endothermic reaction: the temperature is decreased for an exothermic process.arrow_forward
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