Use the given data at 700 K to calculate ΔG°for the reaction
H2(g) + CO2(g) → H2O(g) + CO(g)
Substance | H2(g) | CO2(g) | H2O(g) | CO(g) |
ΔH°f(kJ/mol) | 0 | -393 | -242 | -111 |
S°(J/K·mol) | 131 | 214 | 189 | 198 |
-472 kJ |
||
10.6 kJ |
||
-775 kJ |
||
-2.94 x 104 kJ |
Use the given data at 700 K to calculate ΔG°for the reaction H2(g) + CO2(g) →...
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients. C2H4(g) + H2(g) ----- > C2H6(g) CO (g) + H2O (g) ----- > H2(g) + CO2(g) 3NO2(g) + H2O (l) ----- > 2HNO3(aq) + NO (g) 2SO2(g) + O2(g) -----------> 2SO3(g) 2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H2O (g) Substance --- ΔH° (kJ mol–) --- ΔG° (kJ mol–1) --- S°298 (J K–1 mol–1) C2H4 52.4 86.4 219.3 H2 0 0 130.7 C2H6 -84.0 -32.0 229.2 CO -110.52 -137.15 197.7 H2O -285.83 -237.1 70.0 CO2 -393.51 -394.36 213.8 NO2 33.2 51.30 240.1 NO 90.25 87.6 210.8 SO2 -296.83 -300.1 248.2 O2 0 0 205.2 SO3 -395.72 -371.06 256.76
Use the following data to calculate the value of ΔG°rxn at 298 K for the reaction described by the given chemical equation. Include the units. Compound S°f (J/molK) DH°f (kJ/mol) CO (g) 197.7 –110.5 H2 (g) 130.7 0 CH4 (g) 186.3 –74.6 H2O (g) 188.8 –241.8 CO (g) + 3H2 (g) → CH4 (g) + H2O (g) I got -141.9 KJ/mol, but i think the units are wrong and I don't know why.
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
For the following reaction: 2 CO(g) + O2(g) → 2 CO2(g), given ΔH = -566 kJ and ΔG = -514 kJ, find ΔS (J/K) at 25 oC. Multiple Choices: ΔS = -174 J/K ΔS = -0.174 J/K ΔS = -2.08J/K ΔS = 174 J/K ΔS = -2080 J/K
Use data from the table below to calculate the equilibrium constants at 25∘C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25∘C Substance ΔH∘f(kJ/mol) ΔG∘f(kJ/mol) S∘(J/mol⋅K) H2(g) 0 0 130.7 N2(g) 0 0 191.6 O2(g) 0 0 205.2 NO(g) 91.3 87.6 210.8 NO2(g) 33.2 51.3 240.1 CO(g) -110.5 -137.2 197.7 CO2(g) -393.5 -394.4 213.8 H2S(g) -20.6 -33.4 205.8 S2(g) 128.6 79.7 228.2 1. N2(g)+O2(g)⇌2NO(g)
Given the following thermodynamic data calculate ΔS and ΔSsurr for the following reaction at 25°C and 1 atm. CH4g)+ 2028) CO2g) +2H20(g) So (J/K.mol) 186 205 214 189 ΔΙ!of (kJ/mol) CH4g) 75 02(g) CO2(8) -394 H20(g) -242 J/K J/K Submit Show Hints
CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Use the appropriate table(s) to determine ΔG^o and Keq at 552 degrees C.
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
A) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...