e1ps10 - 1. Rearrange the Gibbs free energy equation ( G =...

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1. Rearrange the Gibbs free energy equation ( G = H - T S) to solve for the temperature at a phase transition. a. T = ( H - G)/ S b. T = H/ S c. T = - G d. T = - G/ S 2. What will happen to vapor pressure when non-volatile solute A is added to a pure solution B? a. Vapor pressure of A increases b. Vapor pressure of B decreases c. Vapor pressure doesn't change d. Boiling point decreases of A inrcreases. e. Boiling point of B decreases 3. Rank the following salts from least to most soluble based on their H hydration : Al 3+ , 4800 kJ; I - , 244 kJ; K + , 350 kJ; Br - , 284 kJ. a. K + < I - < Br- < Al3+ b. Al 3+ < K+ < Br- < I- c. I - < Br - <K + <Al 3+ d. All ions are equally soluble. 4. Which of the following is always true for phase diagrams? a. The slope of the melting curve is always positive b. The critical point will have a lower pressure than the triple point c. Only one phase exists on a phase boundary d. When going from left to right on the graph, pressure and temperature both increase along the condensation curve e. The critical point can be reached at 0K 5. At what temperature will water boil on top of a mountain when normal boiling point is 100C at 1 atm. (You should not need to look at this graph to answer the question) a. Below 100C b. 100C
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c. Above 100C d. Water will not boil 6. Consider a 27 g sample of ice at 1 atm. Initially, the sample is frozen at -20 °C. How much heat must be added to the sample for it to become a liquid at 78 °C. Heat capacity of ice: 2 J/gK. Heat capacity of water: 4 J/gK. ∆H of melting: 330 J/g a. 9.5 kJ b. 18.4 kJ c. 5.3 kJ d. 10.6 kJ 7. As the temperature of a solvent (increases/decreases), the solubility of (some/all) gases increases. a. decreases, all b. increases, some c. decreases, some d. increases, all 8. Rank the following liquids from least to most miscible in H 2 O 2 : H 2 O, C 2 H 6 , CH 2 Cl 2 . a.
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e1ps10 - 1. Rearrange the Gibbs free energy equation ( G =...

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