Calculate AG for the following reaction at 25 °C. C₂H.(g) + 502(g) 3CO2(g) + 4H2O (1) Be sure your answer has the correct number of significant digits. Note: Reference the Thermodynamic properties of pure substances table for additional information. kJ mol Х

a) Briefly describe the Third Law of Thermodynamics.   b) Consider the reaction 2X(g)+ O2(g)→3Y(g) carried out at 25°C and 1 atm. Calculate ΔHrxn°, ΔSrxn°, and ΔGrxn° using the following data. Identify whether the reaction is spontaneous or not. (Assume all gases are perfect).   Substance DHfo (kJ/mol) So(J/k mol) X  (g) -250 250 Y (g) -300 280 O2 (g) 0 205     c) In a reaction, A + B → Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled. Choose the correct rate law for the reaction from below. Explain your answer briefly.   Rate = k[A][B] Rate = k [A][B]2 Rate = k [A]2[B] Rate = k [A][B]3 d) One mole of N2(g) occupies 5 L of volume at 300 K in a sealed cylinder. The gas behaves ideally in expanding isothermally to 10 L. Calculate w, ΔE and ΔH if the expansion proceeds (i) reversibly, (ii) irreversibly against an external pressure at…

The standard reaction free energy AG=-1482. kJ for this reaction: 4 Fe(s) + 30₂(g) 2 Fe₂O3(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 2Fe₂O₂ (s) 4Fe(s) + 30, (g) - Fe(s) + O₂(g) → Fe₂03 (s) Fe₂O₂ (s) → Fe(s) + 0₂ (8) AG kJ kJ X 5

5.)  Which of the following statements accurately describes the spontaneity of the reaction below?Al2O3(s) + 2Fe(s) → 2Al(s) + Fe2O3(s) H°rxn = 830.8 kJ/mol, S°rxn = 168 J/mol·K a. The reverse reaction is always spontaneous.b. The reaction is spontaneous above 4945 K.c. The reaction is spontaneous below 4945 K.d. The reaction is always spontaneous.e. There is not enough information to determine.