The fuel liquid CH₄ is burned with 62 percent theoretical air (38 percent deficiency of air) at 298 K. Products are at 700K and 5 atm Write the combustion equation and find number of moles and a_s and mole fractions of products and using thermodynamic property table (given at the end of the page). Calculate:

A) Molar mass

B) Enthalpy (kJ/kg) and

3. Entropy (kJ/kgK) of the products. Po=1 atm.

CH₄ +a_s/ (O₂+3.76N₂) n1 CO₂+ n2 H₂O +n3 N₂+n4 O₂ +n5 CO+n6 H2