I need help answering 1.1, 1.2, 1.3, and 1.4 at constant pressure

Question 1: Estimate the (1.1) adiabatic flame temperature, (1.2) mole and mass fractions of the products, and (1.3) the higher and the lower heating values for complete constant pressure combustion of a stoichiometric NH3-air mixture. Properties of ammonia are at the nist.gov web book: https://webbook nist.gov/cgi/cbook.cgi?ID = C 7664417&Mask=1 The initial pressure is 1atm and the initial reactant temperature is 298K. Use the following assumptions: 1. Complete combustion (no dissociation) i. e. the product mixture consists of only N2 and H2O. 2. The product mixture enthalpy is estimated using a constant specific heat estimated at a temperature of 1200K. (1.4) How would the estimates (of (1.1) adiabatic flame temperature, (1.2) mole and mass fractions of the products, and (1.3) the higher and the lower heating values) change if the 2nd assumption above regarding a constant specific heat is not made