Question

640 g of oxygen gas, O2, ondergo reversible isothermal expansion at 35°C from a volume of 2.4 to 17.3 m. Assuming ideal gas behaviour, what is the total work performed by the gas? A particular reaction has a standard molar reaction enthalpy of -4362 kJ mol" and a standard molar reaction entropy of +21.6 J K-1 mol- both at 298 K. What is the thermodynamic equilibrium constant for the reaction at 298 K? (Note, rounding errors will have a profound effect of the value calculated.) For the following reaction: 2 N2O5 (8) + 4 NO2 (g) + O2 (g) the initial rate of formation of O, was found to be 1.25 x 10-4 mol dm5-1. What is the initial rate of consumption of N205? A gas is contained in a horizontal cylinder with a moveable piston of cross-sectional area 0.33 m². The region outside the cylinder is at standard ambient temperature and pressure, 298 K and 1 bar. When 2040 J of heat flow into the gas, the internal energy of the gas increases by 1380 J. Calculate the distance through which the piston moves. You may assume friction is negligible.

Answer 1

For a nevensible expansion work V2 w=- net en given, T=35°c = (273735) K = 308 Vi = 214 m3 V2 = 17,3 m 3 W n= n 640 = 64o mole 32 = 20 mole i W = -20 X 81314 X 308 xen 17.3 2.4 =-10116013 J = - 101.16 kg