2. Given the following reaction: 2CH2OH(g) + 302(g) → 2CO2(g) + 4H2O(g) Delta Gº Kj/mol -163...
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 572 kJ -801 kJ -572 kJ 801 kJ
Estimate ∆Gº at 750.0 K for the reaction SO2(g) + 3CO(g) → COS(g) + 2CO2(g) given that at 25.00 ºC ∆Hº=–300.8 kJ/mol and ∆Gº=–246.3 kJ/mol. A –756.7 kJ/mol B –163.7 kJ/mol C –119.6 kJ/mol D –246.3 kJ/mol E –54.5 kJ/mol
For the following reaction: 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH3OH (l) -238.40 127.19 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 H2O (l) -285.83 69.91 Determine the temperature (to two decimal places in K) such that the reaction is in equilibrium in its standard states.
Let’s combust octane. (2C8H18 + 25O2 --> 16CO2 + 18H2O) delta G C8H18= 16.4 kj/mol, delta G CO2 = -394 kj/mol, delta G H2O = -229 kj/mol a. Please calculate the free energy of rxn for the burning of octane. b. Now give the lnKeq at STP. c. Next, give the lnKeq at 200C d. Follow with the free energy of reaction at this temperature
Determine AGº for the overall reaction as written below. Use the summation (E) equation and do not omit the liquid. Is the reaction spontaneous? How can you tell? (9 pts) 2CH2OH(lig) + 302(g) = 2CO2(g) + 4H2O(g) AGE =-166.2 kJ for CH2OH(lig) AGE" =- 394.4 kJ for CO2(g) AGE" =-228.6 kJ for H2O(g)
3. Given the following data: C2H2 (8) +5/2O2(g) → 2CO2 (g) + H20 (1) = - 1300. KJ C(s) + O2(g) → CO2 (g) = -394 kJ H2(g) + 1/2O2(g) → H20 (1) = -286 kJ Calculate for the reaction 2C(s) + H2(g) → C2H2 (8)
Find the enthalpy of combustion of C2H4(g), C2H4(g) + 302(g) → 2CO2(g) + 2H2O(1) given the following data: AHºf[C2H4(g)] = 52 kJ/mol; -285.8 kJ/mol AHºf[CO2(g)]=-393.5 kJ/mol ; AHºf[H2O(1)] = -1331 kJ/mol -731 kJ/mol .BO 2287 kJ/mol .CO -1410.6 kJ/mol.Do
Part A Consider a fuel cell that uses the reaction C2H4 (g)302(g) -2CO2(g) 2H20(1 Using the standard free energies of formation, what is the value of E° for the cell reaction? Substance and StateAG C2H4(g) CO2 (g) (kJ/mol) 68.1 -394.4 H20() O2(g) -237.2 0 Express your answer with the appropriate units. HA ? Value Units E° Previous Answers Request Answer Submit
E2C.6(a) for the reaction C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(g), delta U knot = -1373 kj/mol at 298 k. calculate delta H knot of reaction.