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 Consider the reaction: 2 NOCl(g) ≤ 2 NO(g) + Cl2(g). At 25 ˚C, a particular mixture has equilibrium pressures of P(NOCl) = 1.2 atm, P(NO) = 1.25x10-2 atm and P(Cl2) = 3.0x10-1 atm. Calculate the equilibrium constant Kp. a, 3.26x10-5 The following reaction is investigated: 2 N2O(g) + N2H4(g) ≤ 3 N2(g) + 2 H2O(g) At equilibrium, 0.06 moles of N2O remained after 0.10 moles of N2O and 0.25 moles of N2H4 were placed in a 10 L container. How many moles of N2 were present at equilibrium? c, 0.06 moles 2 NO2(g) ≤ N2O4(g); Kc for this reaction is 7.5 at a certain temperature. If 1.0 mole of NO2 is placed in a 1 L container and allowed to come to equilibrium at this temperature, what will the equilibrium concentration of N2O4 be (in moles per liter)? a, 0.387 M Consider the following equilbrium: H2(g) + I2(s) ≤ 2 HI(g) The proper Kc equilibrium constant expression is: d, [HI]e^2/[H2]e Consider the following reaction at equilibrium: N2(g) + 3 H2(g) ≤ 2 NH3(g) + 92.94 kJ/mole N2 Which of the following changes will shift the equilibrium to the right, favoring products? 1. increasing the temperature 5. removing some NH3 2. decreasing the temperature 6. adding some NH3 3. increasing the pressure 7. removing some N2 4. decreasing the pressure 8. adding some N2 e, 2,3,5,8 The equilibrium constant of the reaction: 2 HCl(g) ≤ H2(g) + Cl2(g) is 4.17x10-34 at 25 °C. What is the equilibrium constant of the reaction: 2 H2(g) + 2 Cl2(g) ≤ 4 HCl(g)? d, 5.75x10^66 At 700 ˚C, the equilibrium concentration of NH3(g) was 0.68 M when the initial concentrations of N2, H2 and NH3 were 2.0 M, 4.0 M and 0 M, respectively. Calculate the equilibrium constant of the reaction: N2(g) + 3 H2(g) ≤ 2 NH3(g) c, 1.1x10-2 HCOOH + Br2 æ CO2 + 2 Br- + 2 H+ When formic acid was mixed with bromine at 25 ˚ C, [Br2] decreased from 8.46x10-3 M at t = 100 s to 5.96x10-3 M at t = 300 s. Calculate the average reaction rate in the 100 to 300 s time interval. e, 1.25x10-5 Ms-1 Identify the correct statement about rate laws. A) the concentrations of all reactants must appear in the rate law B) the rate law is an expression relating the rate of a reaction to the rate constant and reactant concentrations C) the kinetic order of a reactant may be predicted from its stoichiometric coefficient in the balanced chemical equation D) rate laws are predicted theoretically, not measured experimentally E) the rate law describes how the rate depends on temperature b, NH4+(aq) + NO2-(aq) æ N2(g) + 2 H2O(l) Rate = k[NH4+][NO2-] When [NH4+] = 0.01 M and [NO2 -] = 0.15 M the reaction between ammonium and nitrite ions proceeds at a rate of 4.5x10-7 Ms-1. Calculate the rate constant k of this reaction. c, 3.0x10-4 M-1s-1