A cup of rather dilute hot tea initially at 140 degrees F is served to a customer at Howard Johnson's. Unfortunately, before they get around to drinking it, it has spontaneously cooled off to 100 degrees F. Whenever a process takes place spontaneously, there is "free energy" available for the taking if you are clever enough to figure out how to extract it. What is the maximum amount of work you could extract from the cooling process. The temperature of the restaurant (the surroundings) is 70 degrees F. The tea has a mass of 200g.

Given the data in the table in the figure at 1 atm and 25.0 °C, calculate the standard heat of reaction, ∆H°₂₅, for the reaction Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)   A) 216.8 kJ are evolved per mole B) 88.0 kJ are evolved per mole C) 88.0 kJ are absorbed per mole D) 216.8 kJ are absorbed per mole

Which of the following can NOT be deduced from the value of ArGº for a reaction? Select one: the total energy that is absorbed or released by the system during reaction. the value of the equilibrium constant, K, for the reaction. the amount of work that can be obtained from or is required for a reaction or process under standard conditions. the direction (forwards or reverse) of the spontaneous overall reaction.

Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g)  , ∆Horxn = -236.0 kJ

The value of ΔE for a system that performs 190 kJ of work on its surroundings and gains 250 kJ of heat is in kj?

What is the maximum amount of useful work that could possibly be obtained at 25 °C and 1 atm from the combustion of 47.9 g of natural gas, CH4(g), to give CO₂(g) and H₂O(g)? Express your answer as a positive value. kJ