# Calculating Heat Release from Bomb calorimeter

When $$0.400\ \mathrm g$$ $$\ce{CH4}$$ is burned in excess oxygen in a bomb calorimeter that has a heat capacity of $$3245\ \mathrm{J/^\circ C}$$ a temperature increase of $$6.795\ \mathrm{^\circ C}$$ is observed. What is the value of $$Q_V$$?

I thought it was the regular $$Q=mc\Delta T$$ problem but it isn't and not only that I did the equation but it didn't work.

I am not sure what to do right here at the moment

Using the data determine standard enthalpy change for the combustion of methane

Also I would like the definition of the standard enthalpy change and what it tells you and the purpose of it.

Heat of combustion is the amount of heat (enthalpy) liberated when 1 mole $$\ce{CH4}$$ reacts (combusts) with oxygen.
$$\ce{CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)}$$