Final answer:
The heat produced by combustion of 125 g of methanol can be calculated using the molar mass of methanol and its molar enthalpy of combustion, both of which need to be provided to perform the calculation.
Step-by-step explanation:
The question is concerned with the heat of combustion of methanol (CH3OH). Under standard conditions, the combustion of methanol produces energy, which can be quantified in kilojoules (kJ).
To determine how much heat is produced by the combustion of 125 g of methanol under standard state conditions, you would use the molar enthalpy of combustion for methanol, which is the amount of heat released when one mole of methanol is burned completely in excess oxygen at standard conditions.
However, the molar mass of methanol and its molar enthalpy of combustion must be known or provided to perform this calculation. Typically, this information can be found in standard chemical reference materials or textbooks.
As an example, if the molar enthalpy of combustion for methanol is known to be X kJ/mol (where X is a specific numerical value), and the molar mass of methanol is 32.04 g/mol, the calculation would proceed as follows:
- Calculate moles of methanol: (125 g) / (32.04 g/mol)
- Multiply moles of methanol by the molar enthalpy of combustion: moles of methanol × X kJ/mol
This process would give the total heat produced in kJ. Without the exact enthalpy value (X kJ/mol), it isn't possible to give a precise answer to the question.