If the heat of combustion for a specific compound is -1250.0 kJ/mol and its molar mass is 35.39 g/mol, how many grams of this compound must you burn to release 352.40 kJ of heat?

1250.0 kJ/mol x # mol = 352.40 kJ

Solve for # mols.
Then mol = grams/molar mass. You know mols and molar mass, solve for grams.

To solve this problem, we need to use the concept of stoichiometry, which relates the amount of reactants and products in a chemical reaction.

Before we begin, we should convert the molar mass from grams to kilograms by dividing it by 1000:
Molar mass = 35.39 g/mol = 0.03539 kg/mol

Now, let's set up the stoichiometric ratio based on the given information:
- The heat of combustion for the compound is -1250.0 kJ/mol.
- The heat released is 352.40 kJ.

We can use these two values to set up a proportion:
(-1250.0 kJ/mol) / (0.03539 kg/mol) = (352.40 kJ) / (x grams)

Now we can solve for 'x,' which represents the number of grams of the compound we must burn to release 352.40 kJ of heat.

Let's perform the calculations step by step:
(-1250.0 kJ/mol) / (0.03539 kg/mol) = (352.40 kJ) / (x grams)
Simplifying the left side:
-1250.0 / 0.03539 = 352.40 / x

Now cross-multiply:
-1250.0x = 0.03539 * 352.40
x = (0.03539 * 352.40) / (-1250.0)

Simplifying the right side:
x = 0.01240 grams

Therefore, you would need to burn approximately 0.01240 grams of the compound to release 352.40 kJ of heat.