[ahawk1]

im so lost and dont know where to start can someone walk me through this problem and stay with me on here until i figure it out?
Calculate the mass of methane that must be burned to provide enough heat to convert 110.0 g of water at 28.0°C into steam at 114.0°C. (Assume that the H2O produced in the combustion reaction is steam rather than liquid water.)

[ARGOS++]

Dear ahawk1;

The problem and also the result "splits" into three main parts:

• A.)   Determine the molar heat of methane combustion (∆H°_Comb):
  Use a balanced reaction equation (RxN),
  and:    http://en.wikipedia.org/wiki/Standard_enthalpy_change_of_formation
  and:    http://en.wikipedia.org/wiki/Standard_enthalpy_change_of_formation_(data_table)#Miscellaneous_Compounds
  
  
• B.)   Determine the required heat(∆H°_Water) for converting 110g Water of 28°C into steam of 114°C:
  Use:  q_i = c * m *  ∆T      and:   ∆H°_Water  =  q_water + q_evap + q_steam,
  and:     http://www.engineeringtoolbox.com/water-thermal-properties-d_162.html
  
  
• C.)    Finally solve the equation:    x mole * ∆H°_Comb + ∆H°_Water = 0    for  x mole!
  (This holds because no heat is lost everywhere!)

Can you start with A.) or B.) and tell where the troubles occur?

Good Luck!
                    ARGOS⁺⁺