The entropy change for the process                                      H2 O(s) ⟶ H2 O(l)is 22.1 J/K and requires that the surroundings transfer 6.00 kJ of heat to the system. Is the process spontaneous at −10.00 °C? Is it spontaneous at +10.00 °C?

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).

The law of thermodynamics states that every spontaneous process moves towards greater ontropy. second first O third O fourth

For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?

For the reaction 2 A(g) → A2(g), Q = -20.00 kJ for the formation of onemole of A2(g) at constant volume and a temperature of 25.00◦C. If we did thissame reaction at constant pressure, what would be the values of Q, W, ∆U,and ∆H for the formation of one mole of A2(g) at a temperature of 25.00◦C?

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.