find the temperature increase in C expected for 1.00 L of water when it absorbs all of the energy from the combustion of 1.00 g of acetylene, C2H2(g). (Every mole of acetylene releases 1300KJ of energy when combusted)

Answer 1

2C2H2 + 3O2 ==> 2CO2 + 2H2O

dH = 1300 kJ/mol C2H2
How many mols C2H2 do we have? That's mols g/molar mass = 1.0/26 = approx 0.038 but you should redo that since it is an estimate.
The q = dH = mass H2O x specific heat H2O x delta T. Solved for dT.