An important source of copper is from the copper ore, chalcocite, a form of copper(I) sulfide. When heated, the Cu2S decomposes to form copper and sulfur described by the following equation:Cu2 S(s) ⟶ Cu(s) + S(s)(a) Determine ΔG°298 for the decomposition of Cu2S(s).(b) The reaction of sulfur with oxygen yields sulfur dioxide as the only product. Write an equation that describes this reaction, and determine ΔG°298 for the process.(c) The production of copper from chalcocite is performed by roasting the Cu2S in air to produce the Cu. By combining the equations from Parts (a) and (b), write the equation that describes the roasting of the chalcocite, and explain why coupling these reactions together makes for a more efficient process for the production of the copper.

Calculate the equilibrium constant at 10.7 °C for each of the following reactions from the value of ΔG° = 56.1 kJ.I2(s)+Cl2(g)⟶2ICl(g)

17.28 From each equation and standard enthalpy, predict whether the reaction will be spontaneous at all temperatures, spontaneous at low temperatures but nonspontaneous at high temperatures, nonspontaneous at low temperatures but spontaneous at high temperatures, or not spontaneous at any temperature. Explain the reasons. (a) 2HgO(s) 2Hg(l) + O2(g) = 90.8 kJ → (b) 4Fe(s) + 302(g) → 2Fe2O3(s) AH = -1648.4 kJ (c) N2(g) + 3Cl2(g) → 2NC13(g) днө — 460 kJ 作答 (d) 2NH4NO3(s) → 2N2(g) + 4H2O(g) + O2(g) AH® = -225.5 kJ

Calculate ΔG°rxn, ΔH°rxn, and ΔS°rxn of the following reaction: 2O3(g) -> 3O2(g)

Can you help me show the process in this problem? Thermodnamics Calculate ΔG° at 25 °C for the following fermentation reaction: C6H12O6 (aq) à 2C2H5OH (aq) + 2CO2 (g) Ans: -241.6 kJ/mol

The vapor pressure of solid CO2 (dry ice) is 280. torr at −90. °C and 105 torr at −100. °C. (a) What is the value of ΔG° for the reaction CO2(s)  CO2(g) at each temperature? ΔG° at −90 °C        1.52 kJ/mol ΔG° at −100 °C       2.85  kJ/mol (b) What are ΔH° and ΔS° for the reaction CO2(s)  CO2(g) at these temperatures? Assume that ΔH° and ΔS° are constant over this temperature range. ΔH°      26  kJ/mol ΔS°        J/K·mol  need delta S not(c) A dry ice bath is used routinely in the laboratory to keep things cold. It is made by making a power of the dry ice and then mixing the powder with a solvent to make a slurry. Estimate the temperature of the dry ice bath by determining the temperature at which the vapor pressure of CO2 is 1 atm.   (only need delta s part and part c please)

Calculating ΔG under Nonstandard Conditions What is the free energy change for theprocess shown here under the specified conditions?  2NH3(g) ⟶ 3H2(g) + N2(g) ΔG°=33.0 kJ/mol T = 25 °C, PN2 = 0.870 atm, PH2 = 0.250 atm, and PNH3 = 12.9 atm

What is the standard free-energy change ΔG° at 25°C for the following reaction? See the Supplemental Data for ΔGf° data. C(graphite) + 2 Cl2(g) → CCl4(l)   A)  kJ/molB) Calculate the value of the thermodynamic equilibrium constant

a) Write a balanced equation for the gaseous reaction be-tween N₂O₅ and F₂ to form NF₃ and O₂. (b) Determine ΔG°ᵣₙₓ.(c) Find Gᵣₙₓ at 298 K if P(N₂O₅)=P(F₂) = 0.20 atm, P(NF₃) =0.25 atm, and P(O₂) =0.50 atm