A weak acid has a pH of 12.7. Calculate the pOH of the solution. (Give your answer to 1 decimal place)

The change in Gibbs Free Energy, ΔG°, and change in enthalpy, ΔH°, are measured for a reaction to be ΔG° = 63.2 kJ mol^-1, and ΔH° = 278 kJ mol^-1 at a temperature of T = 332.5 K. Calculate the change in entropy, ΔS°, for the reaction. Give your answer in J K^-1 mol^-1.

For a chemical reaction, ΔG > 0 and ΔH > 0. Choose the correct statement below:

When 16.6 g of KCl is added to 210 g of water in a ‘coffee cup calorimeter’, the temperature increases from 20.58 °C to 21.2 °C. Calculate the heat transferred assuming the specific heat capacity of the solution is the same as pure water (4.184 J g^-1 K^-1). Enter your answer in joules (J). 

Predict the sign for the entropy change, ΔS, for the following reaction 

CO₂ (g)   +   H₂O (l)    ⇌   H₂CO₃ (aq)

A syringe contains gas at high pressure. The plunger is released and the gas expands by a total volume of 194 mL so that the pressure inside the syringe equals the pressure of the atmosphere (take as 1.01 x 10² kPa). Assuming ideal gas behaviour and constant temperature, calculate the amount of work done by the gas in the syringe in joules (J).

Which of the following molecules has the highest entropy?

Sodium bicarbonate reacts with acids to give a salt and carbonic acid (H₂CO₃). Carbonic acid rapidly decomposes into water and carbon dioxide. If the release of CO₂ results in 148 J work, and 207 J of heat is transferred to the water, calculate the total change in internal energy accompanying this reaction in joules (J).