3C.3 An FCIO3 molecule can adopt four orientations in the solid with negligible difference in energy. What is its residual molar entropy?

Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K.                2 H(g) ⇌ H"(g)    or equivalently    H(g) + H(g) ⇌ H2(g)             Δf?° (kJ mol-1)                                ?° (kJ K-1 mol-1) H(g)         218.0                                                          0.115 H2(g)           0                                                             0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.

3. A particular protein heat denatures with a melting temperature Tm = 332 K with an enthalpy of unfolding, AHm = 372 kJmol-¹. (a) What is the entropy of unfolding in kJ mol-1 K-1 at Tm? (b) If ACp is 6.6 kJ mol-1 K-1, at what temperature does the free energy of unfolding (AG unfolding) have the greatest value (i.e. the native state is most stable)? (c) Calculate the value of AG and K at this temperature.

5. One might imagine that a reluctant pair of Diels-Alder reactants (diene and dienophile) could eventually be forced to react in high conversion by increasing the temperature. What might prevent the higher temperature from getting the job done. Think about the equation DG = DH - TDS. What the heck is entropy?

For the reaction Na2CO3 (s) + 2HCI9) NaCle) + CO2 (9) + H2O AH is -144.1 kJ. What is AU.

2. In a non-ideal binary mixture of A and B, the chemical potential of A is (a) The partial derivative of the total Gibbs free energy, with respect to the number of moles of A. (b) The partial derivative of the Gibbs free energy of A, with respect to the number of moles of A. (c) The partial derivative of the Gibbs free energy of B, with respect to the number of moles of A. (d) The total Gibbs free energy, divided by the number of moles of A. (e) The Gibbs free energy of A, divided by the number of moles of A.

The enthalpy of sublimation of calcium at 25 °c is 178.2 kJ mol- 1.How much energy (at constant temperature and pressure) must be supplied as heat to 5.0 g of solid calcium to produce a plasma (a gas of charged particles) composed of Ca2+ ions and electrons?

Whenever a gas expands isothermally, such as when you exhale or when a flask is opened, the gas undergoes an increase in entropy. A sample of methane gas of mass 15 g at 260 K and 105 kPa expands isothermally and (a) reversibly, (b) irreversibly until its pressure is 1.50 kPa. Calculate the change in entropy of the gas.

(b) Calculate the increase in entropy when 1.00 mol of a monatomic perfect gas with Cp,m = (5/2)R is heated from 300 K to 600 K and simultaneously expanded from 30.0 L to 50.0 L.

For the following reaction: C2H4(g) + 302(g) → 2CO2(g) + 2H2O(1) What is the change in free energy in J? The relevant standard free energies of formation are: mol kJ AGƒ, C₂H4 = 68.4 mol kJ AG₤. 0, = 0 mol kJ AG, co, = = -393.3 mol kJ AG, H₂O = -285.8 mol •⚫ Your answer should include three significant figures.