Practice Questions for Exam 2 CH 1020 Spring 2017

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1 Practice Questions for Exam 2 CH 1020 Spring Pick all of the statements which are true about a reaction mechanism?. A rate law can be written from the molecularity of the slowest elementary step.. The final rate law can include intermediates.. The rate of the reaction is dependent on the fastest step in the mechanism. V. A mechanism can never be proven to be the correct pathway for a reaction. 2. Consider the reaction: 2A(g) + B(g) 2C(g) When the concentration of substance B in the reaction is doubled (all other factors held constant), it is found that the rate of the reaction remains unchanged. The most probable explanation for this observation is that: A. The reactant with the smallest coefficient in the balanced equation usually has little or no effect on the rate of reaction. B. Substance B is probably a catalyst which means that its effects on the rate do not depend on its concentration C. Substance B is not involved in the ratedetermining step of the mechanism, but is involved in other steps. D. Substance B is not involved in any of the steps in the mechanism of the reaction. 4. Which of the following is a catalyst for this reaction? A. NO 2 B. Cl 2 C. Cl D. NO 2 Cl E. There is no catalyst in this mechanism. 5. What is the rate law for this mechanism? A. Rate = k[no 2 ][Cl 2 ] B. Rate = k[no 2 ] 2 [Cl 2 ] C. Rate = k[no 2 ][Cl] D. Rate = k[no 2 Cl][Cl] E. Rate = k[no 2 Cl] 2 6. Which is the best progress of reaction diagram for the reaction? A. C. B. D. For the next four questions, consider the following proposed mechanism for an exothermic reaction. NO 2 + Cl 2 NO 2 Cl + Cl NO 2 + Cl NO 2 Cl (slow) (fast) 3. Which of the following is a reaction intermediate? A. NO 2 B. Cl 2 C. Cl D. NO 2 Cl E. There is no intermediate. 7. H for an uncatalyzed reaction is 5.0 kj/mol. f the activation energy, Ea, is 20.0 kj/mol, which reaction has the larger activation energy? A. the forward reaction B. the reverse reaction C. both reactions occur at the same rate D. The reaction will not take place without a catalyst.

2 Practice Questions Exam 2 Spring 2017 Page 2 of 6 8. Consider the reaction and its rate law: 3A + B 2C rate = k[a] 3. Which will not increase the rate of reaction? A. ncreasing the concentration of A B. Adding a suitable catalyst C. ncreasing the temperature D. ncreasing the concentration of B E. All will increase the rate. 9. An aqueous reaction occurs by the following mechanism: Step 1: A 2 X 2 + Y A 2 X + XY Step 2: A 2 X 2 + XY A 2 X + X 2 + Y An increase in the concentration of compound Y will result in a(n) [decrease/increase] in the activation energy of the reaction which will result in a(n) [decrease/increase] in the reaction rate. Compound Y is a(n) [reactant/product/intermediate/catalyst]. 10. The reaction profile represents the following chemical equation: A + B C + D Calculate the activation energy (E a ) and H of the reaction at 200 K kj 11. A radioisotope decays to give an alpha particle and Pb-208. What was the original element? 12. When Ra decays, it emits 2 α particles, then a β particle, followed by an α particle. The resulting nucleus is: A Bi 212 D. 85 B E C The, as yet unnamed, superheavy element Uuq was made by firing a beam of Ca-48 ions at Pu-242. How many neutrons are produced in the reaction? 14. What nuclear process involves the splitting of a heavier nuclide into smaller nuclides? 15. The nuclear reaction that takes place in our sun is. The nuclear reaction which can be used to produce heat for the generation of electricity is. 16. What type of radiation do you think the isotope He-6 would emit and why? A. positron emission; n:p ratio too low B. positron emission; n:p ratio too high C. beta emission; n:p ratio too low D. beta emission; n:p ratio too high 17. All of the following would be expected to be stable except 500 kj 200 kj E a H A. 700 kj 300 kj B. 700 kj +300 kj C kj 300 kj D kj +300 kj E. 300 kj 700 kj F. 300 kj +700 kj A. Ne 20 D. O 16 B. Es 243 E. Ca 40 C. He What type of decay would you expect for the unstable nuclide in the previous question? A. alpha decay B. fission C. beta decay D. fusion E. positron emission

3 Practice Questions Exam 2 Spring 2017 Page 3 of What type of radioactive emission should be expected for Al? A. 1 H D. 0 e 1 1 B. 0 e 1 E. 4 He 2 C. None, its stable. 20. What is the binding energy (in J/mol) for Mo-98 (nuclear mass = amu)? Assume that the mass of a neutron is amu and the mass of a proton is amu. Recall that 1 J = 1 kg m 2 /s What amount of energy, in kj, is released when a mole of Co-57 undergoes electron capture? Recall that 1 J = 1 kg m 2 /s Co + 1e 26 Fe mass of nucleus Co-57: mass of nucleus Fe-57: mass of electron: amu amu amu 22. A 1.00 g sample of carbon from wood at an archeological dig in Arizona gave 7900 disintegrations in a period of 20 hours. n the same period, 1.00 g of wood from a modern source underwent 18,400 disintegrations. About how old is the sample, to two significant figures? (The half-life of C 14 is 5730 years.) 23. A 9.9 gram sample of iodine 131 is stored for exactly 3 weeks. f the decay constant is day 1, what mass of the isotope remains? 24. For the hypothetical reaction, 2A(s) + B(g) 3C(g) write the equilibrium constant expression. 25. K c = 2 for the reaction X(g) + Y 2 (g) XY(g) + Y(g) Which of the reaction mixtures below represents a mixture at equilibrium? Assume that dark spheres represent Y atoms and light spheres represent X atoms A. Mixture 1 C. Mixture 3 B. Mixture 2 D. None of the above 26. f K c = 46.9 at 700 K for the reaction, PCl 5 (g) PCl 3 (g) + Cl 2 (g) what is K c for the reverse reaction? 27. What is the value of Kp for the reaction shown in Question 26? 28. n which of the following situations will K eq change? A. when reactant concentrations change B. when temperature is changed C. when product concentrations change D. when a catalyst is added 29. Consider the following reaction at 1700 C. 2CH 4 (g) C 2 H 2 (g) + 3H 2 (g) nitially, the reaction mixture contains only [CH 4 ] = M. At equilibrium, the mixture contains [C 2 H 2 ] = M. What is the equilibrium constant for this reaction at 1700 C?

4 Practice Questions Exam 2 Spring 2017 Page 4 of f K c = 1.70 x 10 3 for the reaction, N 2 (g) + O 2 (g) 2 NO(g) and the initial concentrations are [N 2 ]= M, [O 2 ] = M, and [NO] = M, what is required for the reaction to reach equilibrium? A. Nothing, because the reaction is already at equilibrium. B. More NO must form. C. More O 2 must form. D. A catalyst must be added. 31. The diagram to the left represents an equilibrium mixture for the reaction shown. What can be said about the mixture to the right? 34. At a certain temperature the equilibrium constant, K c, equals 0.11 for the following reaction: 2 Cl 2 (g) + Cl 2 (g) What is the equilibrium concentration of Cl if 0.25 mol of 2 and 0.25 mol of Cl 2 are initially mixed in a 2.0 L flask? 35. A decrease in volume will have what effect on the reaction below? C(s) + H 2 O(g) CO(g) + H 2 (g) A. K decreases B. more CO(g) and H 2 (g) are produced C. no effect D. more H 2 O(g) produced E. K increases 36. Consider the following reaction: CO(g) + 2H 2 (g) CH 3 OH(g) At room temperature, K is approximately , but at a higher temperature K is substantially smaller. Which of the following is true? A. The system is at equilibrium. B. The system is not at equilibrium the forward reaction predominates. C. The system is not at equilibrium, the reverse reaction predominates. 32. For the reaction: 2 H(g) H 2 (g) + 2 (g), K c = at 720 K. f the initial concentrations of H, H 2, and 2 are all M at 720 K, which one of the following is correct? A. The system is at equilibrium. B. The concentrations of H 2 and 2 will decrease as the system is approaching equilibrium. C. The concentration of H will decrease as the system is approaching equilibrium. A. The reaction is endothermic. B. The value of K c for this reaction is smaller at all temperatures. C. At the higher temperature, more CH 3 OH(g) is produced. D. The reaction is exothermic. E. The reaction becomes spontaneous at higher temperatures. 37. What is ΔG for the reaction below at 25 C if ΔG = kj and the partial pressures of the gases involved in the reaction are 10 atm SO 2, 100 atm O 2, and 1.0 atm SO 3? 2SO 2 (g) + O 2 (g) 2SO 3 (g) 33. Consider the following reaction at 100 C. N 2 O 4 (g) 2NO 2 (g) K c = 0.36 A reaction mixture at 100 C initially contains [NO 2 ] = M. What is the equilibrium concentration of NO 2?

5 Practice Questions Exam 2 Spring 2017 Page 5 of Consider the following gas-phase reaction of A 2 (grey spheres) and B 2 (black spheres) molecules. A 2 + B 2 2AB Which of the following reaction mixtures (not at equilibrium) has the largest (most positive) G of reaction? 40. For the reaction below, S = 269 J/(mol K) and H = kj/mol. Calculate the equilibrium constant at 25 C. 3C(s) + 4 H 2 (g) C 3 H 8 (g) A. Mixture D. Mixtures and B. Mixture E. Mixtures and C. Mixture 39. What is G for the vaporization of hydrazine, N 2 H 4, at 70 C if 2.0 mol of hydrazine liquid are present and the pressure of the hydrazine gas is 0.15 atm? N 2 H 4 (l) N 2 H 4 (g) G f = 159 kj/mol for N 2 H 4 (g) G f = 149 kj/mol for N 2 H 4 (l)

6 USEFUL NFORMATON [A] t = kt + [A] 0 ln [A] t = kt + ln[a] 0 1/[A] t = kt + 1/[A] 0 t ½ = [A]0 2k t ½ = ln 2 k 1 t ½ = [A] k 0 E = mc 2 c = m/s J = kg m 2 s 2 1 mol = particles 1 amu = kg K p = K c (RT) n R = L atm mol 1 K 1 G = G o + RT ln Q G o = RT ln K R = J/K mol

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