Consider the reaction H2(g) + Br2(g) ⇌ 2HBr(g) where ΔHo = 2103.8 kJ. In a particular experiment, 1.00 atm of H2(g) and 1.00 atm of Br2(g) were mixed in a 1.00-L flask at 25oC and allowed to reach equilibrium. Then the molecules of H2 were counted by using a very sensitive technique, and 1.10 × 1013 molecules were found. For this reaction, calculate the values of K, ΔGo, and ΔSO.
Answer to relevant QuestionsAt 1500 K the process is not spontaneous. However, the process is spontaneous at 1500 K. Explain. Calculate the entropy change for the vaporization of liquid methane and hexane using the following data: Compare the molar volume of gaseous methane at 112 K with that of gaseous hexane at 342 K. How do the differences in ...Consider a 2.00-mole sample of Ar at 2.00 atm and 298 K. a. If the gas sample expands adiabatically and reversibly to a pressure of 1.00 atm, calculate the final temperature of the gas sample assuming ideal gas behavior. b. ...Consider the system A(g) → B(g) at 25oC. a. Assuming that GoA = 8996 J/mol and GoB = 11,718 J/ mol, calculate the value of the equilibrium constant for this reaction. b. Calculate the equilibrium pressures that result if ...Impure nickel, refined by smelting sulfide ores in a blast furnace, can be converted into metal from 99.90% to 99.99% purity by the Mond process. The primary reaction involved in the Mond process is Ni(s) + 4CO(g) ⇌ ...
Post your question