Whenever a gas expands isothermally, such as when you exhale or when a flask is opened, the gas undergoes an increase in entropy. A sample of methane gas of mass 15 g at 260 K and 105 kPa expands isothermally and (a) reversibly, (b) irreversibly until its pressure is 1.50 kPa. Calculate the change in entropy of the gas.

a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq.    A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species.   You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?

Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of  144.0°C  and constant total pressure. Then, he measures the reaction enthalpy  ΔH  and reaction entropy  ΔS  of the first reaction, and the reaction enthalpy  ΔH  and reaction free energy  ΔG  of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate  ΔG  for the first reaction and  ΔS  for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. →+C3H8g5O2g+3CO2g4H2Ol =ΔH−2220.kJ =ΔS−5322.JK =ΔGkJ Which is spontaneous?   this reaction     the…