2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) ΔH° = -1199 kJ
How many kilojoules are liberated by the combustion of 56.4 g of methanol?
1199 kJ x (56.4g/2*molar mass CH3OH) = ?
Well, 56.4 g of methanol is quite a "mole-ful"! Let's first calculate the number of moles of methanol we have. The molar mass of methanol (CH3OH) is 32.04 g/mol.
So, we divide the mass (56.4 g) by the molar mass (32.04 g/mol) to get the number of moles: 56.4 g / 32.04 g/mol = 1.761 mol.
Now, since the stoichiometric coefficient of methanol (CH3OH) is 2, we'll multiply the moles of methanol by 2 to get the moles of CO2 formed: 1.761 mol * 2 = 3.522 mol.
Finally, we can calculate the energy liberated using the given ΔH° value: -1199 kJ/mol * 3.522 mol = -4212.078 kJ.
So, the combustion of 56.4 g of methanol liberates approximately -4212.078 kJ of energy. That's a real hot topic!
To find out how many kilojoules are liberated by the combustion of 56.4 g of methanol, we need to use the given ΔH° value and convert the grams of methanol to kilojoules of energy released.
Step 1: Calculate the molar mass of methanol (CH3OH)
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.008 g/mol
Molar mass of O = 16.00 g/mol
Molar mass of CH3OH = (12.01 * 1) + (1.008 * 4) + 16.00 = 32.04 g/mol
Step 2: Convert grams of methanol to moles
Number of moles = mass / molar mass
Number of moles = 56.4 g / 32.04 g/mol ≈ 1.7629 mol
Step 3: Calculate the energy released in kilojoules
Energy released = ΔH° * number of moles
Energy released = -1199 kJ/mol * 1.7629 mol
Approximately, Energy released = -2111 kJ
Therefore, approximately 2111 kilojoules are liberated by the combustion of 56.4 g of methanol.
To find out how many kilojoules are liberated by the combustion of 56.4 g of methanol, we need to use the equation and the given heat of reaction.
First, we need to calculate the number of moles of methanol. The molecular weight of methanol (CH3OH) is calculated by adding the atomic weights of carbon (C), hydrogen (H), and oxygen (O):
Molecular weight of CH3OH = (1 * 12.01 g/mol) + (4 * 1.01 g/mol) + (1 * 16.00 g/mol)
= 32.04 g/mol
Next, divide the given mass of methanol (56.4 g) by the molecular weight to find the number of moles:
Number of moles of methanol = 56.4 g / 32.04 g/mol
≈ 1.76 mol (rounded to two decimal places)
Now, we can use the balanced equation and the heat of reaction to calculate the energy liberated during the combustion of methanol:
1 mol of methanol produces -1199 kJ
Therefore, 1.76 mol of methanol will produce:
Energy liberated = 1.76 mol * -1199 kJ/mol
≈ -2110.24 kJ
≈ -2110 kJ (rounded to the nearest kilojoule)
Hence, approximately 2110 kilojoules are liberated by the combustion of 56.4 g of methanol.