Methanol, CH3OH (l), combusts according to the following equation: 2 CH3OH (l) + 3 O2 (g)...
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 amount of non-expansion work that could theoretically be extracted from the cell per mole of methanol combusted? Explain.
(b) What is the minimum amount of heat (per mole of methanol combusted) which must flow to the surroundings in the above fuel cell? Explain.
Homework Answers
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Methanol, CH3OH (l), combusts according to the following
equation:
2 CH3OH (l) + 3 O2 (g)...
10. Given the themochemical equation for the combustion of methanol. 2 CH3OH(g) + 3 O2(g) ®...
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.
1) Consider the equilibrium of methanol vapor and the liquid. CH3OH(l)↽−−⇀CH3OH(g) Thermodynamic Table at 25 ∘C Subst...
1) Consider the equilibrium of methanol vapor and the liquid. CH3OH(l)↽−−⇀CH3OH(g) Thermodynamic Table at 25 ∘C Substance ΔHf∘ (kJ/mol) S∘ (J/mol‑K) ΔGf∘ (kJ/mol) CH3OH(l) −239.2 126.8 −166.6 CH3OH(g) −201.0 239.9 −162.3 What is the vapor pressure of the methanol at −30 ∘C? Pvap= atm What is the vapor pressure of the methanol at 40 ∘C? Pvap= 2) Substance ΔG°f(kJ/mol) M2O(s) −8.70 M(s) 0 O2(g) 0 Consider the decomposition of a metal oxide to its elements, where M represents a generic...
Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l), ΔH°rxn =...
Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l), ΔH°rxn = –1454 kJ/mol. A) How much heat, in kilojoules, is given off when 150.0 g of methanol is burned? [ Select ] B) How many grams of CO2 are produced when the amount of heat determined in part A is released? [ Select ] Molar masses: CH3OH = 32.04 g/mol O2 = 32.00 g/mol CO2 = 44.01 g/mol H2O = 18.02 g/mol
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4...
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4 kJ/mol C(graphite) + O2(g) → CO2(g) ΔHorxn = –393.5 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔHorxn = –285.8 kJ/mol Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l) Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines. From...
For the following reaction: 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Compound ΔH°f (kJ mol-1)...
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.
When methanol, CH3OH , is burned in the presence of oxygen gas, O2 , a large...
When methanol, CH3OH , is burned in the presence of oxygen gas, O2 , a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH ( g ) + 3/2 O2 ( g ) ⟶ CO2 ( g ) + 2H2O ( l ) Δ H = − 764 kJ How much methanol, in grams, must be burned...
When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this r...
When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ How much methanol, in grams, must be burned to produce 807 kJ of heat? mass in grams:
1. 1) luciferin+O2 ⇌ oxyluciferin+light 2) ATP⇌AMP+PPi ΔG∘=−31.6 kJ/mol If the overall ΔG∘ of the coupled...
1. 1) luciferin+O2 ⇌ oxyluciferin+light 2) ATP⇌AMP+PPi ΔG∘=−31.6 kJ/mol If the overall ΔG∘ of the coupled reaction is -1.21 kJ/mol , what is the equilibrium constant, K, of the first reaction at 11∘C? Round your answer to 3 significant figures. 2. When methanol (CH3OH) is combusted, such as when in a gasoline blend, the following reaction occurs: 2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g) Based on the standard free energies of formation given, what is the standard free energy change for this reaction? Report the answer...
For the following chemical reaction DH = -1453 kJ: 2 CH3OH(l) + 3 O2(g) ---> 2...
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
The standard cell potential for the fuel cell 2 H2(g) + O2(g) ⇔ 2 H2O(l) is = +1.23 V at 298 K and +1.18 at...
The standard cell potential for the fuel cell 2 H2(g) + O2(g) ⇔ 2 H2O(l) is = +1.23 V at 298 K and +1.18 at 358 K. Estimate the standard entropy change of the cell reaction.
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