Updated: Dec 30, 2019
Sixth workshop with Dineli for Physical Chemistry (CHEM 3321) with Dr. Nielsen at UT Dallas!
WORKSHOP WITH DINELI | October 8, 2019
Problem 1 – chemical reaction
Using tabulated ∆fH◦ 298 (Table 19.2) and standard molar entropies given in Table 21.2, calculate ∆rxnG◦ 298 for the reaction H2O(`)→H2(g) + 1 2O2(g) At what temperature would the reaction become favorable assuming ∆rxnH◦ 298 is independent of temperature?
Problem 2 – derivative manipulations
Starting from Equation 22.34, show that
(a) Using Table 26.1 find KP for the following reaction at 298 K and 1 bar N2O4(g) → 2NO2(g) (b) Solve for ξ, the extent of reaction, assuming one mole of reactant and no product is initially present.
Using the data in Table 19.2 find KP and KC for the reaction in problem 1 at 1000 K and 1 bar. Rationalize your answer in terms of Le Chatelier’s Principle.
At 900 K, the reaction C2H6(g) → C2H4(g) + H2(g) has ∆H◦ = 24.42 kcal/mol and ∆G◦ = 5.35 kcal/mol. Calculate the percent H2 present at equilibrium if pure C2H6 is passed over a dehydrogenation catalyst at this temperature and 1 atm pressure. (b) Estimate the percent H2 at equilibrium at 1000 K.
Suppose that we have a mixture of the gases H2(g), CO2(g), CO(g) and H2O(g) at 1260 K, with P(H2) = 0.3 bar, P(CO2) = 0.5 bar, P(CO) = 2.5 bar and P(H2O) = 0.5 bar. Is the reaction described by the equation H2(g) + CO2(g) → CO(g) + H2O(g) KP = 1.59 at equilibrium under these conditions? If not what direction will the reaction proceed to attain equilibrium?