6H 2 O A 2 B 3 C 5 D 8 E 10 C162s15e3v1 5 11 E o volts X 2 2e X 013 Y 2 2e Y

6h 2 o a 2 b 3 c 5 d 8 e 10 c162s15e3v1 5 11 e o

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6H 2 O A. 2 B. 3 C. 5 D. 8 E. 10
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C162s15e3v1 5 11 E o (volts) X 2+ + 2e - X 0.13 Y 2+ + 2e - Y 0.44 Z 2+ + 2e - Z 0.76 Which of the following is true under standard conditions? A. Z 2+ ions oxidize X metal B. Y metal reduces Z 2+ ions C. Y is a better reducing agent than Z D. Z 2+ ions are better oxidizing agents than X 2+ ions E. X 2+ ions oxidize Y metal 12 AgBr(s) Ag + (aq) + Br - (aq) K sp = 5.3 × 10 -13 Ag + (aq) + 2NH 3 (aq) Ag(NH 3 ) 2 + (aq) K f = 1.7 × 10 7 When NH 3 is added to AgBr(s), a combination of these two reactions occur: AgBr(s) + 2NH 3 (aq) Ag(NH 3 ) 2 + (aq) + Br - How many moles of AgBr can dissolve in 1.0 L of 2.5 M NH 3 ? A. 0.012 mol B. 3.4 × 10 -7 mol C. 2.4 × 10 -5 mol D. 7.5 × 10 -3 mol E. 0.048 mol 13 Calculate Δ S ° univ for the following reaction at 100 °C CO(g) + H 2 O(g) " CO 2 (g) + H 2 (g) H ° = -41 kJ S ° (J/mol · K) CO(g) 200 H 2 O(g) 199 CO 2 (g) 214 H 2 (g) 131 A. 18 J/K B. 56 J/K C. -54 J/K D. 33 J/K E. 7.0 J/K
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C162s15e3v1 6 14 Consider the galvanic cell based on the following reaction: 2Al(s) + 3Fe 2+ (aq, 2.0 M) 2A1 3+ (aq, 0.030M) + 3Fe(s) E ° cell = 1.22 V Calculate E cell for this cell. A. 1.44 V B. 1.55 V C. 1.44 V D. 1.32 V E. 1.26 V 15 When solid barium fluoride, BaF 2 , is placed in enough water to make 1.5 L of solution, it is found that 1.97 g of BaF 2 (molar mass 175.3 g/mol) dissolves to reach equilibrium at 25 ° C. Calculate K sp for BaF 2 at 25 ° C. A. 1.4 × 10 -5 B. 5.6 × 10 -5 C. 2.2 × 10 -4 D. 4.2 × 10 -7 E. 1.7 × 10 -6 16 N 2 (g) + 3H 2 (g) 2NH 3 (g) Δ G f o = -16.4 kJ/mol for NH 3 Calculate Δ G at 298 K for this reaction when: p N 2 = 0.012 atm, p H 2 = 0.050 atm, and p NH 3 = 3.00 atm A. -33 kJ B. -21 kJ C. +5.9 kJ D. -6.5 kJ E. +13 kJ 17 What is W in Boltzmann's formula, S = k ln W ? A. a fraction indicating the probability of obtaining a result B. a random number C. the number of microstates describing the system D. work times Avogadro’s number E. number of particles in the system
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C162s15e3v1 7 18 E ° (volts) Ag + + e - Ag(s) 0.80 Pb 2+ (aq) + 2e - Pb(s) -0.13 Based on this data, what is the equilibrium constant for the reaction: Pb(s) + 2Ag + (aq) " 2Ag(s) + Pb 2+ (aq) A. 3.8 × 10 -32 B.
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