2CH3OH(l)+3O2(g)→2CO2(g)+4H2O(g
Part B
Calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, assuming H2O(g) as a product.
Part C
Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g/mL.
Part D
Calculate the mass of CO2 produced per kJ of heat emitted.
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Part B: To calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, we can use the coefficients in the balanced equation and the standard enthalpies of formation of the reactants and products. The standard enthalpy change (ΔH) can be calculated using the formula:
ΔH = ΣΔH_products - ΣΔH_reactants
We are given the equation:
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g)
The standard enthalpy change can be calculated as follows:
ΔH = (2 mol CO2 * ΔHf CO2) + (4 mol H2O * ΔHf H2O) - (2 mol CH3OH * ΔHf CH3OH) - (3 mol O2 * ΔHf O2)
The standard enthalpies of formation (ΔHf) for CO2, H2O, CH3OH, and O2 can be found in a thermochemical table.
Part C: To calculate the heat produced by combustion per liter of methanol, we need to consider how much heat is generated when 1 mol of methanol undergoes combustion. We can use the balanced equation and the molar mass of methanol to calculate the heat produced.
First, convert the density of methanol to mass:
Density of methanol = 0.791 g/mL
Volume of 1 L = 1000 mL
Mass of 1 L of methanol = (0.791 g/mL) * (1000 mL) = 791 g
Next, we need to convert the mass of methanol to moles:
Molar mass of methanol (CH3OH) = (12.01 g/mol * 1) + (1.01 g/mol * 4) + (16.00 g/mol + 1) = 32.04 g/mol
Moles of methanol in 791 g = 791 g / 32.04 g/mol = 24.67 mol methanol
Finally, to calculate the heat produced, we need to multiply the moles of methanol by the enthalpy change (ΔH) from Part B:
Heat produced = 24.67 mol methanol * ΔH
Part D: To calculate the mass of CO2 produced per kJ of heat emitted, we first need to convert the heat produced from Part C to kJ:
Heat produced in kJ = Heat produced / 1000
Next, we need to determine the moles of CO2 produced by using the coefficients from the balanced equation. From the equation, we know that for every 2 moles of CO2 produced, 2 moles of CH3OH are consumed.
Moles of CO2 produced = (2 mol CO2 / 2 mol CH3OH) * moles of CH3OH
Finally, we can calculate the mass of CO2 produced using the molar mass of CO2:
Mass of CO2 produced = Moles of CO2 produced * molar mass of CO2
Mass of CO2 produced per kJ of heat emitted = Mass of CO2 produced / Heat produced in kJ
Part B:
To calculate the standard enthalpy change for the combustion of 1 mol of liquid methanol, we need to use the balanced chemical equation provided:
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g)
The standard enthalpy change (∆H°) can be determined by using the standard enthalpies of formation for each of the compounds involved in the reaction.
The standard enthalpy change, ∆H°, is given by the sum of the standard enthalpies of formation of the products, minus the sum of the standard enthalpies of formation of the reactants, multiplied by their stoichiometric coefficients.
The standard enthalpy of formation for a substance is the change in enthalpy that occurs when 1 mole of the substance is formed from its elements, with all substances in their standard states at a given temperature and pressure.
Using the standard enthalpies of formation (∆Hf°):
∆H° = (2 * ∆Hf°(CO2) + 4 * ∆Hf°(H2O)) - (2 * ∆Hf°(CH3OH) + 3 * ∆Hf°(O2))
The standard enthalpies of formation for CO2, H2O, CH3OH, and O2 can be found in a reference table or database.
Part C:
To calculate the heat produced by combustion per liter of methanol, we need to find the number of moles of methanol in 1 liter of methanol.
First, we need to convert the density of methanol from g/mL to g/L. We are given that methanol has a density of 0.791 g/mL.
Density = Mass / Volume
0.791 g/mL = Mass / 1 L
Mass = 0.791 g/mL * 1 L = 0.791 g/L
Next, we need to convert the mass of methanol to moles. To do this, we need to know the molar mass of methanol (CH3OH), which can be found on the periodic table.
The molar mass of CH3OH = 12.011 g/mol (C) + 3 * 1.008 g/mol (H) + 16.00 g/mol (O) = 32.04 g/mol
Now, we can calculate the moles of methanol in 1 L of methanol:
Moles = Mass / Molar mass = 0.791 g/L / 32.04 g/mol = 0.0247 mol/L
Finally, we can calculate the heat produced by combustion per liter of methanol by multiplying the number of moles of methanol by the ∆H° from Part B.
Heat produced per liter of methanol = 0.0247 mol/L * ∆H° (calculated in Part B)
Part D:
To calculate the mass of CO2 produced per kJ of heat emitted, we need to find the moles of CO2 produced and the heat emitted.
First, we need to calculate the moles of CO2 produced from 1 mol of liquid methanol.
Using the balanced chemical equation:
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(g)
From the equation, we can see that 2 moles of CO2 are produced for every 2 moles of CH3OH combusted.
Now, we need to convert the moles of CO2 produced to grams. The molar mass of CO2 can be found on the periodic table.
The molar mass of CO2 = 12.011 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol
Next, we need to calculate the grams of CO2 produced from the moles of CO2.
Grams = Moles * Molar mass = (2 mol CO2 / 2 mol CH3OH) * (44.01 g/mol CO2) = 44.01 g CO2/mol CH3OH
Now, we can calculate the mass of CO2 produced per kJ of heat emitted. We need to convert the heat emitted from kJ to J, and then divide the grams of CO2 by the heat emitted in joules.
Mass of CO2 produced per kJ of heat emitted = (44.01 g/ mol CH3OH) / (Heat emitted in J / 1000)
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B.
dHrxn = (n*dHformation products) - (n*dH formation reactants)
C.
Use density to convert 1L to grams. Then
You know from part B the dH for 1 mol. Convert the mass in grams of 1L CH3OH to mols, the dH/mol x # mols = ?
D.
From part B you know #kJ/2 mol CH3OH and that's the same as the #kJ/2 mol CO2 (from the equation that 2 mol CH3OH = 2 mol CO2). So convert #kJ/2 mol CO2 or #kJ/2*44 g CO2 or #kJ/88g CO2 to 1 kJ/?g CO2