The enthalpy of vaporization of chloroform (CHCl3) is 31.4 kJ/ mol at its boiling point (61.7oC). determine ΔSsys, ΔSsurr, and ΔSuniv when 1.00 mole of chloroform is vaporized at 61.7oC and 1.00 atm.
Answer to relevant QuestionsTwo crystalline forms of white phosphorus are known. Both forms contain P4 molecules, but the molecules are packed together in different ways. The a form is always obtained when the liquid freezes. However, below 276.9oC, ...At 1500 K the process is not spontaneous. However, the process is spontaneous at 1500 K. Explain. Calculate the values of ΔS and DG for each of the following processes at 298 K: H2O(l,298 K) → H2O(g, V = 1000. L/mol) H2O(l,298 K) → H2O(g, V = 100. L/mol) The standard enthalpy of vaporization for water at 298 K is ...At least some of what is in the following quoted statement is false. Change the incorrect statements so that they are correct and defend your answer. What is correct in the statements? What is wrong? Discuss a real world ...Consider the reaction 2CO(g) + O2(g) → 2CO2(g) a. Using data from Appendix 4, calculate K at 298 K. b. What is ΔS for this reaction at T = 298 K if the reactants, each at 10.0 atm, are changed to products at 10.0 atm? ...
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