Verified answer

First find the delta E of water

delta E = (1130g)(4.184J/gC)(65C)

delta E = 307.3148kJ

This is also the delta E of methane.

Now, you have to find the heat of combustion of methane. It will probably be in your textbook

I mole of methane has a heat of combustion of -890.3 kJ mol−1

delta E/heat of combustion

307.3148kJ/(890.3 kJ/mole) = 0.345 moles

0.345 moles x (16.05g/mole) = 5.54g

Methane Ch4

You first need to know the enthalpy of combustion of methane (deltaH = -890 kJ/mol) negative because the reaction is exothermic.

The amount of energy required to heat the water:

E = mass x specific heat capacity of water x change in temperature

= 1.13kg x 4.18 kJ/kg C x 65 C

= 307.0 kJ

Number of moles of methane required:

307.0 kJ / 890 kJ/mol =0.345 mol

Mass of methane required:

mass = number of moles x molar mass

= 0.345 x 16.05 g/mol = 5.54g

What is dH for methane?