What is the ArG for the following reaction (in kJ moll) at 298 K? 2 NO2...
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 A,G for the following reaction (in kJ molt) at 298 K? CH4 (g) + 2 O2(g) = CO2 (g) + 2 H20 (g) The conditions for this reaction are: PCH4 = 1.51 bar Po2 = 1.33 bar Pco2 = 0.21 bar PH2O = 0.62 bar You will also need to use Appendix Il in your textbook (containing standard Gibbs energies of formation).
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? 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
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
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...
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 = 1.40 bar PN2O4 = 1.98 bar
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.
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction the standard change in Gibbs free energy is delta G degree = -72.6 kJ/mol. What is delta G for this reaction at 298 K when the partial pressures are PNO = 0.l00 atm, PO2 = 0.150 atm, and PNO2 = 0.650 atm Number delta G = kJ/mol
Find ΔrG for reaction (in kJ mol-1) at 298 K? 2 NO2 (g) ⇌ N2O4 (g) Given Conditions: Pressure: NO2 = 1.25 bar Pressure: N2O4 = 0.65 bar N2O4(g) --