What is the A,G for the following reaction (in kJ molt) at 298 K? CH4 (g)...
1--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? CH4 (g) + 2 O2 (g) ⇌ CO2 (g) + 2 H2O (g) The conditions for this reaction are: PCH4 = 0.73 bar PO2 = 0.27 bar PCO2 = 0.10 bar PH2O = 1.41 bar 2--What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 =...
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3(g) The conditions for this reaction are: PO2 = 0.62 bar PO3 = 0.33 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). ΔfH ΔfG S * O2(g) 0 0 205.2 O3(g) 142.7 163.2 238.9
What is the ArG for the following reaction (in kJ moll) at 298 K? 2 NO2 (g) = N204 (g) The conditions for this reaction are: PNO2 = 1.59 bar PN204 = 1.41 bar You will also need to use Appendix Il in your textbook (containing standard Gibbs energies of formation). You have 5 attempts at this question.
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌N2O4 (g) The conditions for this reaction are: PNO2 = 0.12 bar PN2O4 = 0.99 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation).
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) ⇌ Si2H6(g) The conditions for this reaction are: PH2 = 1.83 bar PSi2H6 = 0.96 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). ΔGf(Si2H6) = 127.3 kJ/mol ΔGf(H2) = 0 kJ/mol
1.A) What is the equilibrium constant for a reaction at temperature 31.5 °C if the equilibrium constant at 55.4 °C is 1.53? For this reaction, ΔrH = 20.2 kJ mol-1 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". 1B) What is the ΔrG° for the following reaction (in kJ mol-1)? N2(g) + O2(g) + Cl2(g)...
What is the ΔrG° for the following reaction (in kJ mol-1)? 2 NO2 (g) ⇌N2O4 (g) To solve, use Appendix II in your textbook (containing standard Gibbs energies of formation) and use the method of Gibbs energy of formation.
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The conditions for this reaction are: PO2 = 1.64 bar PO3 = 1.28 bar .
12. Methane, a major component in natural gas, can be used as a fuel in combustion reactions (proposed by oil tycoon T. Boone Pickens in an add campaign this past year). What is the maximum amount of work (in kJ) that could be supplied by following reaction under the given conditions at 298 K? CH4 (g) + 2 O2(g) Æ CO2 (g) + 2 H2O (g) where ΔHo rxn = -803 kJ and ΔSo rxn = -4.00 J/K and PCH4...
I keep getting 2.10 as the answer here but it is incorrect. Is there something I am doing wrong? What is the A,G for the following reaction (in kJ mol-1) at 298 K? 2 Si (s) + 3 H2 (g) = SizH6 (g) The conditions for this reaction are: PH2 = 1.41 bar Psi2H6 = 1.20 bar You will also need to use Appendix Il in your textbook (containing standard Gibbs energies of formation). You have 5 attempts at this...