Use the table to calculate an approximate enthalpy or heat of reaction for the combustion of one mole of methane gas (CH4) to form gaseous H2O and CO2. What Volume (in L) of methane is needed to produce 3329 kJ of heat for methane gas at 36 oC and 9.15 atm pressure?

I got 20.7, which is apparently wrong. Any help is appreciated!
The table can be found here: i54. tinypic. com / 25tvp0p (just take out the spaces)

To calculate the volume of methane needed to produce a certain amount of heat, we can use the following steps:

Step 1: Find the enthalpy of reaction for the combustion of one mole of methane.
To do this, we need to refer to the table you provided, which shows the enthalpy change of reaction (ΔH) values. Look for the entry representing the combustion of methane (CH4) to form H2O and CO2. The value in the table represents the enthalpy change per mole of methane combusted.

Step 2: Calculate the number of moles of methane required to produce the given amount of heat.
Use the formula:
q = ΔH * n
where q is the heat provided (3329 kJ), ΔH is the enthalpy change of reaction per mole of methane, and n is the number of moles of methane. Rearrange the formula to solve for n:
n = q / ΔH

Step 3: Convert moles of methane to volume using the ideal gas law.
The ideal gas law is given by:
PV = nRT

Given:
- Temperature (T) = 36 °C = 309 K (convert to Kelvin)
- Pressure (P) = 9.15 atm

The ideal gas law can be rearranged as:
V = nRT / P

Now we can substitute the value of n calculated in Step 2, along with the given values of T, P, and R (ideal gas constant), to calculate the volume.

Please note that without the specific ΔH value from the table, I cannot provide a precise calculation. However, I can guide you through the steps to perform the calculation with the given information.

Write the equation and balance it.

CH4 + 2O2 ==> CO2 + 2H2O
dHrxn = (n*BE reactants)-(n*BE prodicts)
Don't forget to use the O-O bond energy which is listed separately and remember to use O=C=O for CO2.
dHrxn kJ/mol x ?mol = 3329 kJ
Convert ?mol CH4 to L at the conditions listed by using PV = nRT.