Questions 1 13 cover material from Exam 1

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1 Questions 1 13 cover material from Exam 1 1. Which intermolecular forces are present in H Te(l)? A. dispersion only C. dispersion, dipole-dipole, and hydrogen bonding B. dispersion and dipole-dipole D. ion-dipole only. Assuming all compounds are in the liquid phase, which of the following has the compound with the greater surface tension listed first? A. benzene (C 6 H 6 ), H O C. CH 3 Cl, CH 4 B. CH 3 OCH 3, CH 3 CH OH D. Br, I 3. Antimony has a normal boiling point of 1860 K and ΔH vap = kj/mol. What happens to the vapor pressure of antimony when the temperature is increased to 1950 K? A. The vapor pressure exceeds 760 torr. B. The vapor pressure is 760 torr. C. The vapor pressure falls between 760 and 380 torr. D. The vapor pressure falls below 380 torr. 4. Sublimation is A. the phase transition from solid to liquid. B. the phase transition from gas to solid. C. the phase transition from liquid to gas. D. the phase transition from solid to gas.

2 5. How much heat is required to convert 9.01 g of ice at C to liquid water at 0.0 C? Specific heat, ice =.09 J/g. C Specific heat, water = 4.18 J/g. C Specific heat, steam =.01 J/g. C Heat of vaporization, water = 40.7 kj/mol Heat of fusion, water = 6.0 kj/mol A kj C kj B kj D kj 6. What is the density of chromium (5.00 g/mol), which crystallizes in a body-centered cubic unit cell with a volume of cm 3? A. 4.5 g/cm 3 C. 1.1 g/cm 3 B. 9.7 g/cm 3 D g/cm 3 7. What type of crystalline solid has a low melting point and is held together by dispersion forces only? A. molecular solid C. ionic solid B. nonbonding atomic solid D. network covalent solid 8. Which of the following compounds is most soluble in hexane, C 6 H 14? A. NH 3 C. KI B. H O D. CCl 4

3 9. Which statement best describes the unique property of a supersaturated solution? A. A supersaturated solution must have more solute than solvent. B. A supersaturated solution can dissolve more solute. C. A supersaturated solution has more solute dissolved than predicted by the solubility. D. A supersaturated solution has a precipitated solute in equilibrium with the dissolved solute. 10. Oxygen is most soluble in water at A. high temperature and high partial pressure of oxygen. B. low temperature and high partial pressure of oxygen. C. high temperature and low partial pressure of oxygen. D. low temperature and low partial pressure of oxygen. 11. A 1 m HNO 3 aqueous solution contains A. 1 g of HNO 3 in 1.00 L of solution. B. 1 g of HNO 3 in 100 ml of water. C. 1 mol of HNO 3 in 1.00 kg of solution. D. 1 mol of HNO 3 in 1.00 kg of water. 1. What is the freezing point of an aqueous.3 m ethylene glycol solution? The freezing point constant, K f, of water is 1.86 C/m. A C C C B C D..3 C

4 13. Which of the following M solutions will have the lowest osmotic pressure? A. CaCl C. (NH 4 ) 3 PO 4 B. C 6 H 1 O 6 D. NaNO 3 Questions 14 6 cover material from Exam 14. If H (g) appears at a rate of 1.00 M/s at a particular moment in the reaction below, what is the rate of CH 4 (g) consumption at the same instant? CH 4 (g) + H S(g) CS (g) + 4 H (g) A M/s C..50 M/s B M/s D M/s 15. For the reaction NO(g) + Cl (g) NOCl(g) rate = k [NO] [Cl ] what is the effect on the rate if the concentration of NO is tripled and that of Cl is doubled? A. The rate will increase by a factor of eighteen. B. The rate will increase by a factor of six. C. The rate will increase by a factor of twenty-four. D. The rate will decrease by a factor of twelve.

5 16. The decomposition of N O(g) on a Pt surface follows zero-order kinetics. N O(g) N (g) + O (g) Which curve accurately graphs the relationship between rate and concentration for this reaction? A. Reaction 1 C. Reaction 3 B. Reaction D. Reaction When the Kelvin temperature of a reaction is reduced by half, the value of the rate constant, k A. doubles. B. increases, but doesn t necessarily double. C. decreases by half. D. decreases, but not necessarily by half.

6 18. The reaction, Cl(g) Cl (g), is known to be catalyzed by N (g). The following mechanism has been proposed for the catalyzed reaction. Step 1 N + Cl N Cl fast Step N Cl + Cl Cl + N slow What is the rate law for the reaction, Cl(g) Cl (g)? A. rate = k[n Cl] C. rate = k[cl] B. rate = k[n ][Cl] D. rate = k[cl] 19. Which one of the following is the equilibrium constant expression, K c, for the reaction below? ZnS(s) + 3O (g) ZnO(s) + SO (g) A. B. [SO [O [O ] 3 ] ] [SO ] 3 C. D. [ZnO] + [SO ] [ZnS] + 3[O ] [ZnS][O ] [ZnO] [SO ] 3 0. What is K p for the overall reaction that converts propane (C 3 H 8 ) and steam to carbon dioxide and hydrogen gas (H ) at 100 K given the following information? C 3 H 8 (g) + 3 H O(g) 3 CO(g) + 7 H (g) K p = CO(g)+ H O(g) CO (g) + H (g) K p = 0.69 A C B D

7 1. Which way will the reaction proceed, given the following initial concentrations? [C H 4 ] = M, [H O] = 0.00 M, [C H 5 OH] = 0.00 M C H 4 (g) + H O(g) C H 5 OH(g) K c = at 50 K A. to the left because Q > K C. to the right because Q > K B. to the left because Q < K D. to the right because Q < K. For the following reaction at 98 K, K p = NO (g) N O 4 (g) At equilibrium, the partial pressure of NO is 0.1 atm. Determine the partial pressure of N O 4 at equilibrium. A. 15 atm C. 1. atm B atm D atm 3. Given the following reaction, initially at equilibrium, which change will cause the greatest shift in the equilibrium to favor product formation? 3 C(s) + 4 H (g) C 3 H 8 (g) ΔH rxn = 105 kj/mol A. double the mass of C C. remove H B. decrease the pressure of the container D. lower the temperature

8 4. In the following reaction, NH 3 is behaving as a(n). H PO 4 (aq) + NH 3 (aq) HPO 4 (aq) + NH + 4 (aq) A. Brønsted-Lowry acid C. Arrhenius acid B. Brønsted-Lowry base D. Arrhenius base 5. Which one of the following acids has the lowest percent ionization at M? A. HCN, K a = C. HC 9 H 7 O 4, K a = B. HC H 3 O, K a = D. HCl, K a >> 1 6. Which M solution will have the highest ph? A. ketamine, C 13 H 16 ClNO, K b = B. ammonia, NH 3, K b = C. piperidine, C 5 H 10 NH, K b = D. pyridine, C 5 H 5 N, K b =

9 Answer Key: 1. B. C 3. A 4. D 5. A 6. D 7. B 8. D 9. C 10. B 11. D 1. C 13. B 14. A 15. A 16. A 17. D 18. B 19. A 0. C 1. C. B 3. D 4. B 5. A 6. C

CHE 107 FINAL EXAM - PART A July 31, 2013

CHE 107 FINAL EXAM - PART A July 31, 2013 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the