Question

How much methanol, in grams, must be burned to produce 831 kJ of heat?

Answer 1

To find the mass of methanol burned to produce 831 kJ of heat, divide the energy by the enthalpy of combustion for methanol to get the number of moles and then multiply by the molar mass of methanol to convert to grams.

Step-by-step explanation:

To calculate how much methanol needs to be burned to produce 831 kJ of heat, we first need to know the enthalpy of combustion for methanol. Unfortunately, this information is not directly provided, but let's assume we have a hypothetical value that one mole of methanol upon combustion releases 'x' kJ of heat. The standard molar mass of methanol is approximately 32.04 g/mol.

First, we determine the number of moles of methanol that would release 831 kJ of heat using the equation:

1. Calculate the moles of methanol by dividing the desired heat energy (831 kJ) by the enthalpy of combustion (x kJ/mol).
2. Moles of methanol = 831 kJ / x kJ/mol.

Next, we convert the moles of methanol to grams using the molar mass of methanol:

1. Convert moles to grams: Moles of methanol × 32.04 g/mol.

With these steps, you can determine the mass of methanol in grams required to produce 831 kJ of heat.