The change in the Gibbs energy of a certain constant-pressure process is found to fit the expression AG/J = -73.1 + 42.8(T/K). Calculate the value of AS for the process.
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- Calculate the change in Gibbs energy for each of the sets of ΔrH∘, ΔrS∘, and T. predict wether or not it will be spontaneous at the temprature indicatedCalculate (a) the (molar) Gibbs energy of mixing, (b) the(molar) entropy of mixing when the two major componentsof air (nitrogen and oxygen) are mixed to form air at 298 K.The mole fractions of N2 and 0 2 are 0.78 and 0.22. respectively. (c) Is the mixing spontaneous?Calculate (a) the (molar) Gibbs energy of mixing, (b) the (molar) entropy of mixing when the two major components of air (nitrogen and oxygen) are mixed to form air at 298 K. The mole fractions of N2 and O2 are 0.78 and 0.22, respectively. (c) Is the mixing spontaneous?
- Calculate the change in Gibbs energy for each of the sets of ΔrH∘, ΔrS∘, and T.The standard Gibbs energy of formation of rhombic sulfur is zero and that of monoclinic sulfur is +0.33 kJ mol-1, at 25 °c.Which polymorph is the more stable at that temperature?The standard Gibbs energy of formation of gaseous ozone at 25.0 ℃ ΔfGo, is162.3 kJ. mol-1, for standard state of 1 bar. The reaction is: 3O2 (g) ⇌ 2O3(g). Calculate the value of Kx at 2 bar.
- Calculate the change in S when one mole of water is heated from 263 to 283 K given the molar capacities inJ.K-1 , Cp(ice) = 2.09 + 0.126T, Cp(water)=75.3, and change in Hm=6000Jmol-1The standard Gibbs energy of formation of rhombic sulfur is zero, and that of monoclinic sulfur is +0.33 kJ mol−1 at 25 °C. The standard molar entropy of rhombic sulfur is 31.80 J K−1 mol−1, and that of monoclinic sulfur is 32.6 J K−1 mol−1. At what temperature will the transition occur at 1 bar? _______ K. 3 sig. fig.Use the fundamental equation of therodynamics here tocalculate the change Gibbs energy when 3.1 mmol N_2(g) occupying 3.0L at 350 K expandsisothermally to 15 L.
- Suppose a certain small bird has a mass of 30 g. What is the minimum mass of glucose that it must consume to fly to a branch 10 m above the ground? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide and water vapour at 25 °C is -2828 kJ.The difference in a chemical potential of a particular substance between two regions of a system is -9.5 kJ/mol. By how much does the Gibbs energy change when 0.30 mmol of that substance is transferred from one region to the other?Give typed explanation not a single word hand written otherwise leave it liquid benzene has a Gibbs energy of 124.3kj/mol at 1atm and 298K. What is the chemical potential for liquid benzene at 388K?