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tutor packet-mcfinal - General Chemistry Dept Tutor 8:00...

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General Chemistry Dept Tutor Pina Patel / Justin Rheem 8:00 – 9:50 pm at SSH 100 Chemistry 1C Final Review Packet 1. Balance the following redox reactions a. Fe 2+ (aq) + MnO 4 - (aq)→ Fe 3+ (aq) + Mn 2+ (aq) (in acidic solution) b. Ag(s) + CN - (aq) + O 2 (aq) → Ag(CN) 2 - (aq) (in basic solution) c. Cr 2 O 7 2- + CH 3 OH(aq) → CH 2 O(aq) + Cr 3+ (aq) (in acidic solution) d. Cl 2 (g) → Cl - (aq) + OCl - (aq) (in acidic solution) 2. a. Sketch and calculate the voltage produced by the following electrochemical cells. Your sketch should label the anode, cathode, material composing each, solution composition at each, salt bridge, and direction of electron flow. Assume all concentrations are 1.0 M and pressures at 1.0 atm Cl 2 + 2e- → 2 Cl - E°= 1.36 V Br 2 + 2e- → 2 Br- E°= 1.09 V b. Calculate ΔGº and K at 25 C for the reaction above. 3. M(s) + Cd 2+ (aq) M + (aq) + Cd(s) a. The reduction potential for M(s) must be less than a certain value. What is that value if the reduction potential for Cd 2+ is -0.40 V.
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General Chemistry Dept Tutor Pina Patel / Justin Rheem 8:00 – 9:50 pm at SSH 100 b. Write the two half reactions, and identify which takes place at the anode and which takes place at the cathode. 4. Of the following pairs, which has the greater entropy? Explain each choice. a. 1 mole gaseous hydrogen atoms or 0.5 mole gaseous hydrogen molecules? b. 1 g dew or 1 g frost c. “Perfect” diamond or flawed diamond, each ¼ carat? d. 5 mL liquid ethanol at 0 ° C or 5mL liquid ethanol at 50 ° C? 5. Calculate the pressure of O 2 (in atm) over a sample of NiO at 25°C if ∆G° = 212 kJ/mol for the reaction NiO (s) ↔ Ni (s) + ½ O 2 (g) 6. The equilibrium constant (K p ) for the reaction is 4.40 at 2000 K. H 2 (g) + CO 2 (g) ↔ H 2 O (g) + CO (g) (a) Calculate ∆G° for the reaction.
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General Chemistry Dept Tutor Pina Patel / Justin Rheem 8:00 – 9:50 pm at SSH 100 (b) Cacluate ∆G for the reaction when the partial pressures are P H2 = 0.25 atm, P CO2 = 0.78 atm, P H20 = 0.66 atm, and P CO = 1.20 atm. 7. 2C(s) + 2H 2 (g) C 2 H 4 (g) H° rxn = 52.3 kJ/mol and rxn = -53.07 JK/mol at 298 K. This reaction is spontaneous at: a) No temperature b) Temperatures below 1015 K c) Temperatures above 985 K d) Temperatures below 985 K e) All temperatures 8. A solution is made by mixing 5.00 x 10 2 mL of 0.167 M NaOH with 5.00 x 10 2 mL 0.100 M HCOOH. Calculate the equilibrium concentrations of H + , HCOOH, HCOO - , OH - , and Na + . 9. A volume of 75 mL of 0.600 M NaF is mixed with 25 mL of 0.15 M Sr(NO 3 ) 2 . Calculate the concentrations in the final solutions of NO 3 - , Na + , Sr 2+ , and F - . (K sp for SrF 2 = 2.0 x 10 -10 .) 10. Calculate whether or not a precipitate will form if 2.00 mL of 0.60 M NH 3 are added to 1.0 L of 1.0 x 10 -3 M FeSO 4.
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tutor packet-mcfinal - General Chemistry Dept Tutor 8:00...

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