How to find the Heat of Formation in this problem

When 10.00 g of phosphorus is burned in O2(g) to form P4O10(s), enough heat is generated to raise the temperature of 2920 g of water from 18.0 degrees C to 38.0 degrees C.
Calculate the heat of formation of P4O10(s) under these conditions. (in kJ/mol)

Thank you so much everyone for your help! :)

Heat generated = spht. H2O x m x delta t =4.18 J/gC x 2920 g x 20.0 C = 244000 J
mole P4 = 10.0 g P4 x 1 mole P4/ 124 g P4 = 0.0806 moles
? kJ/mole = 244 kJ/0.0806 mole = 3030 kJ/ mole

from the equation
4P + 5O2 ---> P4O10
10.00 g / 30.97 g/mol = 0.3229 mol of P
then it's 4 to 1 over to P4O10 giving 0.08072 mol
now the enerqy
Q = m c delta(T) = 2.920 kg (4.1813 kJ/(kg*C) (20.0 C) = 244.2 kJ
finally
heat of formation is in kJ/mol
Ho = 244.2 kJ / 0.08072 mol = 3025 kJ/mol