Consider the relationship
The equilibrium constant for some hypothetical process was determined as a function of temperature (in kelvins) with the results plotted below.
From the plot, determine the values of ΔHo and ΔSo for this process. What would be the major difference in the ln(K) versus 1/ T plot for an endothermic process as compared to an exothermic process?
Answer to relevant Questionsa. Use the equation in Exercise 86 to determine ΔHo and ΔSo for the autoionization of water: H2O(l) ⇌ H+(aq) + OH-(aq) b. Estimate the value of ΔGo for the autoionization of water at its critical temperature, 374oC. A 1.50-mole sample of an ideal gas is allowed to expand adiabatically and reversibly to twice its original volume. In the expansion the temperature dropped from 296 K to 239 K. Calculate ΔE and ΔH for the gas expansion. Two 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, ...The deciding factor on why HF is a weak acid and not a strong acid like the other hydrogen halides is entropy. What occurs when HF dissociates in water as compared to the other hydrogen halides? 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. ...
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