What is the change in entropy in a large mass of water at 50 °C when it receives 155 kJ of energy in the form of heat? Assume the change is reversible and the mass of water is large enough that the temperature of the water stays constant.

Calculate the change in entropy (in J/K) that occurs in the system when 1.00 mole of diethyl ether(C4H10O) condenses from a gas to a liquid at its normal boiling point (34.6°C).

Calculate the normal boiling point of ethanol (CH3CH2OH) in degrees Celsius, given that its enthalpy of vaporization is 38.6 kJ/mol and its entropy of vaporization is 110 J/(K⋅mol).

Which of the following describes the second law of thermodynamics?deltaS(system) + deltaS (surroundings) <0deltaS (system) - deltaS (surroundings) = 0deltaS(system) - deltaS (surroundings) <0deltaS(system) - deltaS (surroundings) > 0deltaS(system) + deltaS (surroundings) = 0deltaS (system) + deltaS (surroundings) > 0

8. Can a process occur if the entropy of the system decreases and the enthalpy increases?

For a particular reaction at 148.1 °C, delta G=−1428.51 kJ, and       delta S =393.69 J/K  .  Calculate delta G for this reaction at −62.8 °C.   Free energy is related to enthalpy, temperature, and entropy through the equation delta G = delta H -T(delta S) Δ?=Δ?−?Δ? delta H = delta G + T (delta S) Solve for the enthalpy of the reaction. Assume that enthalpy and entropy will not change between the two temperatures. Use the values from the prior scenario (temperature) to determine the new free energy value using the first equation.