If the heat of combustion for a specific compound is -1320.0 kJ/mol and its molar mass is 92.41 g/mol, how many grams of this compound must you burn to release 544.30 kJ of heat?
1320 kJ/mol x (1 mol/92.41) x ?g = 544.30 kJ. Solve for ?g
To solve this problem, we need to use the concept of molar mass and heat of combustion.
1. First, let's calculate the amount of heat released when one mole of the compound is burned. We are given that the heat of combustion is -1320.0 kJ/mol.
2. Next, we need to calculate the number of moles of the compound that would release 544.30 kJ of heat. We can use the equation:
moles = heat released (kJ) / heat of combustion (kJ/mol)
Substituting the given values, we have:
moles = 544.30 kJ / -1320.0 kJ/mol
3. Now, we have the number of moles of the compound. To determine the mass, we can multiply the number of moles by the molar mass.
mass (g) = moles × molar mass
Substituting the values, we have:
mass (g) = moles × molar mass
= (544.30 kJ / -1320.0 kJ/mol) × 92.41 g/mol
Therefore, to find the number of grams of the compound needed to release 544.30 kJ of heat, multiply the moles of the compound by its molar mass.