5 moles of an ideal gas at 300 K expand isothermally from 5 L to 50 L against a constant external pressure of 1 atm. The work done is:

For the reaction 2H2(g) + O2(g) -> 2H2O(g), delta_H = -484 kJ. If this reaction is carried out in a bomb calorimeter (constant volume), the heat evolved at 25 C would be:

The enthalpy of neutralisation of a strong acid with a strong base is approximately:

When 2 moles of C2H6 are completely burned and the water formed is in gaseous state, delta_H is -3000 kJ. Given delta_H_vap(H2O) = 44 kJ/mol, the delta_H when water is formed as liquid is:

For the combustion of methane: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l), delta_H = -890 kJ. The value of delta_U at 25 C is approximately: