If you burn 13.7 g of methane (CH4) burns in oxygen, then 686 kJ is evolved. What is the amount of heat produced per mole of methane burned?

CH4 + 2O2 --> CO2 + 2H2O

So you get 686 kJ for 13.7 g CH4. How much heat will you get for 1 mol (16 g)?
Thats 686 kJ x 16/13.7 = ? kJ

thank you i got 801.1678 is that correct

I think so but you have too many significant figures. If your prof is picky about s.f. s/he will count off points.

To find the amount of heat produced per mole of methane burned, we can use the molar mass of methane and the given amount of heat evolved.

Step 1: Calculate the number of moles of methane burned.
To do this, we need to know the molar mass of methane (CH4), which is the sum of the atomic masses of each element in the compound. The atomic mass of carbon (C) is 12.01 g/mol, and the atomic mass of hydrogen (H) is 1.01 g/mol.

Molar mass of CH4 = (12.01 g/mol) + 4 * (1.01 g/mol) = 16.05 g/mol

To find the number of moles of methane burned, divide the given mass (13.7 g) by the molar mass of methane.

Number of moles of methane burned = 13.7 g / 16.05 g/mol

Step 2: Calculate the amount of heat produced per mole of methane burned.
Now that we know the number of moles of methane burned, we can calculate the amount of heat produced per mole.

Amount of heat produced per mole of methane burned = 686 kJ / (13.7 g / 16.05 g/mol)

Simplifying the equation, we get:

Amount of heat produced per mole of methane burned = 686 kJ / (13.7 / 16.05) mol

Now we can calculate the answer.

Amount of heat produced per mole of methane burned ≈ 806 kJ/mol

Therefore, the amount of heat produced per mole of methane burned is approximately 806 kJ/mol.