SOLVED

11) For the reaction: 2N2O5(g) → 4NO2(g) + O2(g) the rate law is:   = k[N2O5] At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2. At the time when N2O5 is being consumed at a rate of -1.2 × 10-4 M/s, what is the rate at which NO2 is being formed? A) 1.2 × 10-4 M/s B) 2.4 × 10-4 M/s C) 6.0 × 10-5 M/s D) 3.0 × 10-5 M/s E) 4.8 × 10-4 M/s 12) For the reaction: 2N2O5(g) → 4NO2(g) + O2(g) at the time when N2O5 is being consumed at a rate of -1.2 × 10-4 M/s, what is the rate at which O2 is being formed? A) 1.2 × 10-4 M/s B) 2.4 × 10-4 M/s C) 6.0 × 10-5 M/s D) 3.0 × 10-5 M/s E) 4.8 × 10-4 M/s 13) For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3, when the rate of reaction is 2.0 × 10-5, what is the rate of disappearance of KI? A) -0.67 × 10-5 B) -2.0 × 10-5 C) -4.0 × 10-5 D) -6.0 × 10-5 E) -1.0 × 10-5 14) For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3, when the rate of reaction is 2.0 × 10-5, what is the rate of disappearance of C2H4Br2? A) -0.67 × 10-5 B) -2.0 × 10-5 C) -4.0 × 10-5 D) -6.0 × 10-5 E) -1.0 × 10-5 15) For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3, when the rate of reaction is 2.0 × 10-5, what is the rate of appearance of C2H4? A) 0.67 × 10-5 B) 2.0 × 10-5 C) 4.0 × 10-5 D) 6.0 × 10-5 E) 1.0 × 10-5 16) For the reaction: C2H4Br2 + 3 KI → C2H4 + 2 KBr + KI3, when the rate of reaction is 2.0 × 10-5, what is the rate of appearance of KBr? A) 0.67 × 10-5 B) 2.0 × 10-5 C) 4.0 × 10-5 D) 6.0 × 10-5 E) 1.0 × 10-5 17) In the reaction C4H9Cl(aq) + H2O(l) → C4H9OH(aq) + HCl(aq) the concentration of the reactant changes from 0.0562 M to 0.0431 M in 85 sec. What is the average rate of decomposition over this interval? A) 1.54 × 10-4 M/s B) 1.54 × 10-4 moles C) 1.54 × 10-4 moles/s D) 0.0154 M E) 0.0154 M/s 18) Define rate law. A) A theoretical equation that describes how the rate of reaction depends on the concentration of reactants. B) An experimentally determined equation that describes how the rate of reaction depends on the concentration of reactants. C) A theoretical equation that describes how the rate of reaction depends on temperature, orientation and number of collisions. D) An experimentally determined equation that describes how the rate of reaction depends on temperature, orientation and number of collisions. E) A statement that describes how the ratio of reaction depends on concentration of reactants developed from the balanced equation. 19) If a reaction has a rate equation of rate = k[A][B][C] then it is: A) overall second order B) overall first order C) overall third order D) zero order in A E) second order in B 20) The reaction has the rate law Rate = k[A][B]2. Which will cause the rate to increase the most? A) doubling [A] B) lowering temperature C) tripling [B] D) quadrupling [A] E) doubling [B]