3. 4. A mole of argon is allowed to expand adiabatically from a pressure of 10 bar and 298.15 K to 1 bar. What is the final temperature and how much work can be done? Cym=32R. (Answers: 118.7 K; -2238 J) 2 moles of O2 (g) which can be regarded as ideal (Cp = 29.4 J K' mar') is maintained in a volume of 11.2 dm³ at 273 K. (a) If the gas is heated reversibly to 373 K at constant volume. (i) How much work is done on the system? (0J) (ii) What is the increase in internal energy? (iii) How much heat was added to the system? (iv) What is the increase in enthalpy? (4.22 kJ) (4.22 kJ) (5.89 kJ) If the gas is heated reversibly to 373 K at constant pressure. (i) How much work is done by the system? (ii) How much heat is supplied to the system? (iii) What is the increase in enthalpy? (iv) What is the increase in internal energy? (1.66 kJ) (5.88 kJ) (5.88 kJ) (4.22 kJ) mporature of 100 kg of Calculate the amount of heat required to raise the temperature of 1 mol of O2(g) from 298 K to 500 K (a) at constant (atmospheric) pressure (b) at constant volume nC₂dT; (Hints: Consult Tables for the expression for Cp. For (a) dqp = dH = integrate the last expression to obtain the value of AH. For (b), regard O2(g) as behaving ideally and obtain the expression for C, from that for Cp) (Answers: 6.16 KJ; 4.25 kJ) Use the thermochemical equations 2CO2 (g) + H2O(g) ->> C2H2(g) +5/202(g) H2(g) +1/202(g) -> H₂O(g) 2CO2 (g) + 3H2O(g) -> C2H6(g) +7/202(g) AH=+5287.4 kJmol AH-1602.8 kJmol AH= +6367.4 kJmol to determine the standard enthalpy for the following reaction C2H6(g) →C2H2(g) + 2H2(g) (Answer: 2125 kJ mol¹) given that