2. Given the following reaction: 2CH2OH(g) + 302(g) → 2CO2(g) + 4H2O(g) Delta Gº Kj/mol -163...
1. Keq = 8.63x10-4 for a reaction. Which of the following must be true? ∆Gº=0 ∆Gº=1 ∆Gº>0 ∆Gº<0 2. What is the value of Keq if ∆Gº=-9.48 kJ (R=8.314 J/mol-K)? 6700 1.00 1.01 45.9 3. Calculate ∆Gº for the reaction, C3H8(g)+5O2(g)→3CO2(g)+4H2O(g), where ∆Gfº=-23.5 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 600 kJ -600 kJ -2070 kJ 2070 kJ
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
Calculate the heat of reaction in (kJ) for the following reaction: 2CO(g) + O2(g) --> 2CO2(g) given the following data: C + 1/2O2 --> CO(g) delta H= -110.5 KJ/mol C + O2(g) --> CO2(g) delta H= -393.5 KJ/ mol
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