Calculate G° for each reaction at 298K using G°f values.
2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) kJ
Calculate G° for each reaction at 298K using G°f values. 2 CH3OH(g) + 3 O2(g) 2...
AH = -727 kJ Given that CH3OH (1) + 3/2 O2 (g) → CO2 (g) + 2 H2O(1) CO(g) + 1/2O2 (g) → CO2 (9) CH3OH(1) → CH3OH(g) AH = -284 kJ AH = 38 kJ H20 (1)→ H20 (9) AH = 44 kJ what is AH, in kJ, for the reaction CH3OH (g) + O2(g) →CO (g) + 2 H2O (9)
For the following chemical reaction DH = -1453 kJ: 2 CH3OH(l) + 3 O2(g) ---> 2 CO2(g) + 4 H2O(l) How much energy in kilojoules will be released when 250 g of CH3OH undergo combustion? (M.M. (CH3OH) = 32.04) a)11337 kJ b)5669 kJ c)2834 kJ d)726.5 kJ e)1453 kJ
13 Calculate AHo, 298K for the following reaction: CO(g)1/2 O2(g) CO2(g) Given: AHof,298K (in kJ mol-1): CO(g): -110.53 CO2(g): -393.51
10. Given the themochemical equation for the combustion of methanol. 2 CH3OH(g) + 3 O2(g) ® 2 CO2(g) + 4 H2O(l) DrH = −1453 kJ/mol reaction d. Review the units “kJ/mol reaction”. What does “mole reaction” mean? e. If you produce 857 kJ of heat, how many “mole reactions” occurred? f. Relate the energy of the “mole reaction” to moles of methanol and determine the mass (in grams) of methanol needed.
Which of the following the correct expression of Q for the following reaction 2 CH3OH(g) + 3 O2(g) ---> 2 CO2(g) + 4 H2O(l) a. [CH3OH]2[O2]3/[CO2]2[H2O]4 b. [CH3OH]2[O2]3/[CO2]2 c. [CO2]2/[CH3OH]2[O2]3 d. [CO2]2[H2O]4/[CH3OH]2[O2]3 e. (2[CH3OH])(3[O2])/(2[CO2])(4[H2O])
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ
7. Calculate the AHReaction for the reaction 2H2(g) + CO(g) → CH3OH() Using the following equations: CH3OH(1) + O2(g) → C(s) + 2H2O(1) C(s) + O2 (g) — CO(g) H2(g) + O2(g) → H2O(1) AH = -333.00 kJ AH =-111.52 kJ AH = -285.83 kJ
Methanol, CH3OH (l), combusts according to the following equation: 2 CH3OH (l) + 3 O2 (g) → 2 CO2 (g) + 4 H2O (l) ∆rHo (298 K) = −1452 kJ Here is a list of Entropies of formation: S (J K-1 mol-1) at 298 K CH3OH (l) =126.8 O2 (g) = 205.14 CO2 (g) = 213.74 H2O = (l) 69.91 (a) If the above reaction was used in a fuel cell, say, to perform work, what will be the maximum...
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) Calculate ΔH for the reaction using the bond enthalpies given. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) Calculate the overall enthalpy change for this reaction using the bond enthalpies given.
Consider the reaction: 2NO(g) + O2(g)2NO2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.710 moles of NO(g) react at standard conditions. G°rxn = kJ