How many kilojoules are released when 85.0g methanol is burned?

heatreleased=Heatcombusionmethanol*mass

look up the heat of combustion for methanol

To determine the amount of kilojoules released when 85.0g of methanol is burned, you need to use the formula:

q = m × C × ΔT

where:
q = heat released or absorbed (in joules)
m = mass of the substance (in grams)
C = specific heat capacity (in joules per gram degrees Celsius)
ΔT = change in temperature (in degrees Celsius)

Specifically for combustion reactions, the formula can be modified as:

q = m × ΔHc

where:
ΔHc = heat of combustion (in joules per gram)

To find the heat of combustion for methanol, you will need to refer to a reliable source or a database of thermodynamic values. The heat of combustion for methanol is typically reported in units of kilojoules per mole.

Assuming you have the value for the heat of combustion of methanol, you can calculate the heat released:

1. Convert the given mass of methanol to moles by dividing by its molar mass. The molar mass of methanol (CH3OH) is 32.04 g/mol.
moles = mass / molar mass

2. Multiply the moles of methanol by the heat of combustion to calculate the heat released.
q = moles × ΔHc

3. Convert the calculated heat from joules to kilojoules, by dividing by 1000.
q(kJ) = q(J) / 1000

By following these steps, you will be able to determine the amount of kilojoules released when 85.0g of methanol is burned.