physical chemistry - How do I calculate the enthalpy change when a gas is being used to heat water?

The question I'm trying to answer is:

Calculate the mass of butane gas that would be needed to heat $724\ \mathrm{cm^3}$ of water from an initial temperature of $7.44\ \mathrm{^\circ C}$ to $50.7\ \mathrm{^\circ C}$. The thermochemical equation for the combustion of butane is:

$$\ce{2C4H10(g) + 13O2 -> 8CO2(g) + 10H2O(l)}\quad\Delta H=-5748\ \mathrm{kJ/mol}$$

I know that the equation for enthalpy is $$Q=m\times c\times\Delta T$$ and I calculated this for water:

$$Q=724\times4.18\times43.26$$

$$Q=130918.6032$$

I don't know where to go from here in order to figure out the mass of butane needed. Please tell me if I have done something wrong or if you can help me to solve the rest of the problem.