Substract equation (2) from equation (1)
....(3)
Substitute equation (3) in equation (1)
Hence, the temperature at which process occurs reversibly is 300 K.
The change in free energy of a certain process is equal to 4.000 kJ at 400.K...
A certain isothermal and isobaric process is characterized by DG = + 150. kJ at 500. K and and DG = + 350. kJ at 600. K. Assuming DH and DS do not depend on temperature, determine the temperature where the process occurs reversibly and the temperature range where it occurs spontaneously.
A reaction is at equilibrium at 298 K. At 310 K, the Gibbs free energy for the reaction is –12.6 kJ/mol. Assuming that both entropy and enthalpy are independent of temperature, what are the values of the entropy and enthalpy for this reaction?
change in Helmholtz free energy for this process? (-2862 kJ/mol) 7. Calculate the entropy change when 0.7760 moles of oxygen gas, a perfect gas, expands isothermally from a volume of 36.80 mL to 84.90 mLs. (ANS: 5.394 J/K) 8. The standard reaction enthalpy for the hydrogenation of propene, CH2=CHCH + 5O2 →
What is the value for the standard change in Gibbs free energy (in kJ), when the standard change in enthalpy is 284.6 kJ and the standard change in entropy is 189.89 J/K at 25oC?
What is the value for the standard change in Gibbs free energy (in kJ), when the standard change in enthalpy is (-395.2) kJ and the standard change in entropy is (-256.27) J/K at 25oC?
1. If q 60 kJ and w = 96 kJ for a certain process, that process (3) a. requires a catalyst. b. is endothermic. c. occurs slowly. d. is exothermic. e. cannot occur. 2. What is the change in internal energy of the system (AU) if 71 kJ of heat energy is absorbed by the system and 12 kJ of work is done on the system for a certain process? (4) a. 83 kJ b. 59 kJ c. 71 kJ...
The change in Gibbs energy of a certain constant-pressure is found to fit the expression AG/J = -85.40 + 36.5 (T/K) where K is Kelvin temperature unit. i) Calculate the value of AS for the process and ii) AH for the process. (Hint: use the Helmholtz Equation)
Part A: An object at 400 K absorbs 25.0 kJ of heat from the surroundings. What is the change in entropy ?S of the object? Assume that the temperature of the object does not change appreciably in the process. Part B: An object at 500 K dissipates 25.0 kJ of heat into the surroundings. What is the change in entropy ?S of the object? Assume that the temperature of the object does not change appreciably in the process.
Question 5 (2.0 pts) Assume that Cp for an ideal gas is given by co(T) = 0.9 + 2.5 x 10-* T, in kJ/kg-K, where is the temperature in Kelvin. (Use the gas constant R = 0.3 kJ/kg-K) (a) (+0.4) Derive an expression for Cy as a function of temperature. The gas undergoes an isochoric process from a temperature T, = 400 K to T2 = 500 K. Calculate the change in (b) (+0.6) enthalpy, in kJ/kg, (c) (+0.6) entropy,...
The change in Gibbs energy of a certain constant-pressure is found to fit the expression AG/J = -85.40 + 36.5 (T/K) where K is Kelvin temperature unit. i) Calculate the value of AS for the process and ii) AH for the process. (Hint: use the Helmholtz Equation)