Why is it necessary to define a modified standard state for biochemical applications of thermodynamics?

For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g)→ 2FE2O3(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is –824.2 kJ mol. What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASS O -660.4 kJ O -988.0 kJ O -1484.6 kJ O-1812.2 kJ

Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo

Consider Rh(II) and Ti(II). How many microstates are there for each of these ions?

In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) a) Predict the sign of the system entropy change in this reaction and explain your answer. b) Thermochemical data for this reaction are shown below. Use this data to determine the system entropy change. NH3(g) 192.3 -45.9 O₂(g) 205.0 0.0 NO(g) 210.7 90.2 H₂O(g) +188.7 -285.8 Sº / J mol-1 K-1 H₂/kJ mol-¹ c) Use the values in the table to calculate the system standard enthalpy change, AH. d) Use your answers to (b) and (c) to explain why this reaction is feasible at any temperature. e) Use your answer to (c) to calculate the surroundings entropy change in J.mol-¹ K-¹ at 298K.