CH302 Practice Quiz 2 on Kinetics(It will be a miracle if I got all these calculations right--make sure you point out my errors while we work them)1. One of the reactions used commercially to produce ammonia gas is3H2(g) + N2(g) 2NH3(g)A proper expression for the rate of this reaction could be1. -3Δ[ NH3]/ Δ t2. + Δ [ NH3]/3 Δ t3. -2 Δ [ NH3]/ Δ t4. - Δ [ NH3]/2 Δ t5. + Δ [ NH3]/2 Δ t correct2. For the reaction3H2(g) + N2(g) 2NH3(g)Trial[N2][H2]Rate10.20.311.820.40.311.830.40.9318.6Deduce the order with respect to H2, N2, and the rate constant (dimensions left out ofthe latter on purpose) based on the above data.1. 0, 3, 437 correct2. 0, 0, 4373. 1, 2, 1964. 0, 1, 1963. If the rate of a reaction is Rate = k [A]0 then appropriate units for the rate constant k are1. sec2. sec-13. mol-1L sec-14. mol L-1sec -1correct5. L mol-1sec-14. The decomposition of sulfuryl chloride into sulfur dioxide and chlorineSO2Cl2(g) SO2(g) + Cl2(g)has a rate constant of 2.2 x 10-6 sec-1. If one started with a sample containing 2.8 moles of sulfuryl chloride perliter what concentration would be left after 2 days?1. 1.9 M correct2. 0.68 M3. 0.12 M4. 0.052 M5. 0.15 M5. Consider the potential energy diagram shown below.A….B350300250 B kJ 200150100 50 A 0What is the activation energy Ea for the reaction A B?1. 300 kJ correct2. -300 kJ3. 50 kJ4. -100 kJ5. 100 kJ6. Consider the multi-step reaction that has the overall reaction2A + 2B C + DWhat is the rate law expression that would correspond to the following proposed mechanism?A + B I (fast)I + B 2[A] + X (fast)X + A D (slow)1. Rate = k [A] 2 [B]2. Rate = k [[B]3. Rate = k [A] [B]4. Rate = k [A] [B] 25. Rate = k [A] 2 [B] 26. Rate = k [B]2 correct7. Calculate the activation energy of a reaction if the rate constant is 0.014 sec –1 at 1000C and 0.65 sec –1 at2000C?1. 56 J/mol correct2. 68 kJ/mol3. 6.4 kJ/mol4. 77 kJ/molProblem 8. The activation energy1. will increase with increasing temperature.2. will remain constant with changes in temperature correct3. will be larger if the rate constant is larger.4. is part of the change in enthalpy of a reaction5. can be positive or negative in
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