What is the ΔH° for the following reaction (in kJ/mol of reaction exactly as written)? 2 NO2 (g) → N2O4 (g) To solve, use Appendix II in your textbook (containing standard heats of formation).
What is the ΔH° for the following reaction (in kJ/mol of reaction exactly as written)? 2...
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? 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).
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)? Cu2O (s) ⇌Cu (s)+ CuO (s) 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 = 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.
The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 ∘C , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ΔH∘f values might look something like this: Substance ΔH∘f H(g) 218 kJ/mol H2(g) 0 kJ/mol Ba(s) 0 kJ/mol Ba2+(aq) −538.4...
What is the ΔrG° for the following reaction (in kJ mol-1)?C6H12O6 (s, glucose) + 6 O2 (g) ⇌ 6 CO2 (g) + 6 H2O (l)To solve, use Appendix II in your textbook (containing standard Gibbs energies of formation) and use the method of Gibbs energy of formation. A copy of Appendix II has also been posted on eClass.
1. For the equilibrium reaction: 2NO2 - N2O4 a) calculate the literature values of ΔG°, ΔH° and ΔS° for the equilibrium reaction (ΔS° NO2 - 240.4 Jk/mol, N2O4- 304.3 Jk/mol) (ΔG° NO2- 51.839 KJ/mol, N2O4-98.286 KJ/mol) (ΔH° NO2 -33.85 KJ/mol, N2O4- 9.660 KJ/mol) b) From your understanding of the principals of FTIR spectroscopy, why is it that you do not see absorbance peaks for N2 gas but you do see them for NO2 and N2O4?