A sample of ice weighing 18.02 g, initially at 230.0oC, is heated to 140.0oC at a constant pressure of 1.00 atm. Calculate q, w, ΔE, ΔH, and ΔS for this process. The molar heat capacities (Cp) for solid, liquid, and gaseous water— 37.5 JK-1mol-1, 75.3 JK-1mol-1, and 36.4 JK-1mol-1, respectively—are assumed to be temperature-independent. The enthalpies of fusion and vaporization are 6.01 kJ/ mol and 40.7 kJ/ mol, respectively. Assume ideal gas behavior.
Answer to relevant QuestionsCalculate the entropy change for a process in which 3.00 moles of liquid water at 0oC is mixed with 1.00 mole of water at 100.oC in a perfectly insulated container. (Assume that the molar heat capacity of water is constant ...Predict the sign of ΔSsurr for the following processes. a. H2O(l) → H2O(g) b. I2(g) → I2(s) For the reaction 2Al(s) + 3Br2(l) → 2AlBr3(s) ΔSo is equal to –144 J/ K. Use this value and data from Appendix 4 to calculate the value of So for solid alumi-num bromide. The value of ΔGo for the reaction 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) is –5490. kJ. Use this value and data from Appendix 4 to calculate the standard free energy of formation for C4H10(g). Hydrogen cyanide is produced industrially by the following exothermic reaction: Is the high temperature needed for thermodynamic or for kinetic reasons?
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