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A chemist studied the reaction mechanism for the reaction
by reacting N16O with 18O2. If the reaction mechanism is
what distribution of 18O would you expect in the NO2? Assume that N is the central atom in NO3, assume only N16O18O2 forms, and assume stoichiometric amounts of reactants are combined.
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Chapter 18 Solutions
Chemistry: An Atoms First Approach
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- For the reaction A2 + 2B 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B atoms are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forward. 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?arrow_forward
- Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?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_forwardFor the reaction A2 + B2 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B2 molecules are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.arrow_forward
- 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_forwardThe value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.arrow_forwardIn the gas phase, acetic acid exists as an equilibrium of monomer and dimer molecules. (The dimer consists of two molecules linked through hydrogen bonds.) The equilibrium constant, Kc, at 25 C for the monomer-dimer equilibrium 2 CH3CO2H (CH3CO2H)2 has been determined to be 3.2 104. Assume that acetic acid is present initially at a concentration of 5.4 104 mol/L at 25 C and that no dimer is present initially. (a) What percentage of the acetic acid is converted to dimer? (b) As the temperature increases, in which direction does the equilibrium shift? (Recall that hydrogen-bond formation is an exothermic process.)arrow_forward
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