if the heat of combustion for a specific compound is -1320.0 KJ/mol and its molar mass is 67.53 g/mol how many grams of this compound must you burn to release 791.60 kj of heat
1320 0 kJ/mol x ?mol = 791.60 kJ.
Solve for ?mol, then
g = mol x molar mass.
Thank you, it worked... I was diving the wrong way
To find out how many grams of the compound you need to burn to release 791.60 kJ of heat, you need to use the heat of combustion and the molar mass of the compound.
First, calculate the number of moles of heat released by dividing the given heat value by the heat of combustion:
Moles of heat released = 791.60 kJ / (-1320.0 kJ/mol)
Next, to convert moles to grams, you'll need to use the molar mass of the compound:
Grams of the compound = Moles of heat released × Molar mass
Substituting the values into the equation, you get:
Grams of the compound = (791.60 kJ / (-1320.0 kJ/mol)) × 67.53 g/mol
Now, let's calculate the answer:
Grams of the compound = (791.60 × 67.53) / (-1320.0) g
Note that the molar mass has a negative sign since the heat of combustion is also negative.
Simplifying the expression:
Grams of the compound ≈ -40.095 g
Since mass cannot be negative, there seems to be an error in the calculation, as it is not possible to release 791.60 kJ of heat by burning -40.095 grams of the compound. Please double-check the given values or the calculation.