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All Textbook Solutions for Chemistry: Matter and Change
2PP3PP4PP5PP6PP7SSC8SSC9SSC10SSC11SSC12PP13PP14PP15PP16SSC17SSC18SSC19SSC20SSC21SSC22SSC23PP24PP25PP26SSC27SSC28SSC29SSC30SSC31SSC32PP33PP34PP35PP36PP37PP38SSC39SSC40SSC41SSC42SSC43SSC44PP45PP46PP47PP48SSC49SSC50SSC51SSC52SSC40AExplain what is meant by the average rate of a reaction.How would you express the rate of the chemical reaction AB based on the concentration of Reactant A? Howwould that rate compare with the reaction rate based onthe Product B?What is the role of the activated complex in a chemical reaction?Suppose two molecules that can react collide. Underwhat circumstances do the colliding molecules not react?45AIf AB is exothermic, how does the activation energyfor the forward reaction compare with the activationenergy for the reverse reaction (AB) ?In the gas-phase reaction, I2+Cl22ICl,[I2] changesfrom 0.400M at 0.00 min to 0.300M at 4.00 min.Calculate the average reaction rate in moles of I2 consumedper liter per minute.48A49A50AIn general, what is the relationship between reaction rate and reactant concentration?Apply collision theory to explain why increasing the concentration of a reactant usually increases the reaction rate.53A54AApply collision theory to explain why powdered zinc reacts to form hydrogen gas faster than large pieces of zinc when both are placed in hydrochloric acid solution.Hydrogen peroxide decomposes to water and oxygen gas more rapidly when manganese dioxide is added. The manganese dioxide is not consumed in the reaction. Explain the role of the manganese dioxide.57A58A59A60A61A62A63A64A65A66A67A68A69A70A71A72A73A74A75A76A77A78A79A80A81A82A83ADifferentiate between the shaded areas in Figure 16.24at temperatures T 1 and T 2 on the basis of the number ofcollisions per unit time that might occur with energyequal to or greater than the activation energy.Apply the method of initial rates to determine the order of a chemical reaction with respect to Reactant X. Create a set of hypothetical experimental data that would lead you to conclude that the reaction is second order in X.86A87A88ACreate a table of concentrations, starting with 0.100Mconcentrations of all reactants, that you would proposein order to establish the rate law for the reaction aA+bB+cDproducts using the method ofinitial rates.90A91A92A93A94A95A96A97A99A100A101A102A1STP2STP3STP4STP5STP6STP7STP8STPUse the diagram below to answer Questions 8 and 9. Which sample could contain particles of magnesiumfluoride? A. a B. b C. c D. Both a and b10STP11STP12STP13STP14STP15STP16STP17STP18STP19STP1PP2PP3PP4SSC5SSC6SSC7SSC8SSC9SSC10SSC11SSC12SSC13SSC14SSC15SSC16SSC17SSC18SSC19PP20PP21PP22PP23SSC24SSC25SSC26SSC27SSC28SSC29SSC30SSC31PP32PP33PP35SSC36SSC37SSC38SSC39SSC33A34A35A36A37A38A39A40A41A42A43A44A45A46A47A48A49A50A51A52A53A54A55A56A57A58A59A60A61A62A63A64AWhy are compounds such as sodium chloride usually not given Ksp values?66A67A68A69A70A71A72A73A74A75A76A77A78AEvaluate this statement: A low value for Keq means that both the forward and reverse reactions are occurring slowly.80A81A82A83A84A85A86A87A88A89A90A91A92A93A94A95A96A97A98A99A100A101A102A103A104A105A1STP2STP3STP4STP5STP6STP7STP8STP9STP10STP11STP12STP13STP14STP15STP16STP17STP18STP1PP2PP3PP4PP5PP6PP7PP8SSC9SSC10SSC11SSC12SSC13SSC14SSC15SSC16SSC17SSC18PP19PP20PP21PP22PP23PP24PP25PP26PP27SSC28SSC29SSC30SSC31SSC32SSC55AWrite a balanced chemical equation that represents the self-ionization of water.Classify each compound as an Arrhenius acid or an Arrhenius base H2S RbOH Mg(OH)2 H3PO4Geology When a geologist adds a few drops of HCl to a rock, gas bubbles form. What might the geologist conclude about the nature of the gas and the rock?Explain the meaning of the relative sizes of the two shaded areas to the right of the dark vertical line in Figure 18.28.Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.Why can H+ and H3O+ be used interchangeably in chemical equations?