Thermodynamics Test 2 Thermodynamics Test 2 1 / 10Which of the following processes is associated with a decrease in entropy? Melting of ice Boiling of water Sublimation of a solid Condensation of steam 2 / 10The specific heat capacity of a substance is given by cp = A + BT. The amount of heat required to change the temperature of 1 mol of the substance from T1 to T2 at constant pressure is A(T2 - T1) + B(T2^2 - T1^2) 1/2 A(T2^2 - T1^2) + B(T2 - T1) A(T2 - T1) + B/2(T2^2 - T1^2) A(T2 - T1) + B(T2 - T1) 1/2 A(T2^2 - T1^2) + B(T2 - T1) 3 / 10In an adiabatic free expansion of an ideal gas, which of the following is true? w = 0 and q = 0 w < 0 and q = 0 w = 0 and ΔU > 0 w > 0 and q > 0 4 / 10Which of the following conditions ensures a spontaneous reaction at all temperatures? ΔH > 0, ΔS < 0 ΔH 0 ΔH > 0, ΔS > 0 ΔH < 0, ΔS < 0 5 / 10The enthalpy of neutralization of a strong acid and a strong base is approximately constant at -57.3 kJ/mol. What is the reason for this consistency? The reaction is always at equilibrium The reactions are all similar, involving the combination of H+ and OH- ions to form water All strong acids and bases have the same standard molar enthalpy. The heat capacity of water is very high. 6 / 10For a non-spontaneous process, what is the change in Gibbs free energy (ΔG)? ΔG = 0 ΔG > 0 ΔG < 0 ΔG is independent of temperature. 7 / 10A system absorbs 150 J of heat from the surroundings and does 50 J of work on the surroundings. What is the change in the internal energy of the system? 100 -100 200 -200 8 / 10What is the condition for a process to be spontaneous at high temperatures? ΔH > 0 and ΔS < 0 ΔH 0 ΔH > 0 and ΔS > 0 ΔH < 0 and ΔS < 0 9 / 10The change in enthalpy of a reaction is -40 kJ and the change in entropy is -100 J/K. At what temperature (in K) is the reaction at equilibrium? 400 40 4000 0.4 10 / 10What is the value of the molar heat capacity at constant volume (Cv) for a diatomic ideal gas? 3/2 R 5/2 R 7/2 R R Your score isThe average score is 0% 0% Restart quiz
