1. The problem statement, all variables and given/known data The following reaction takes place at standard conditions 4NH3(g)+6NO(g)----->5N2(g)+6H20 A)calculate reaction enthalpy and Gibbs reaction energy B)Calculate Kp 2. Relevant equations the table gives the following values for deltaG0f[X] NH3(g)=-16.5 Kj/mol NO(g)=87.6 KJ/mol H20(g)=-228.6 KJ/mol ln(Kp)=-deltaG/(RT) 3. The attempt at a solution I finished part a) and found gibbs reaction energy to be -1815 KJ For part b) i am unsure of what to enter for deltaG in the equation ln(Kp)=-deltaG/(RT). Do I use the reaction energy calculated from part a), deltaG for NH3, NO, or H20? Any help is appreciated, thanks!