Question

Il. Results The objective of this experiment is to calculate the enthalpy of foermation for NH.CKs) (Reminder-beat of formation is the ΔΗ for the formation of one mole of a compound from the elements.) Write the balanoed chemical equation for the formation of 1 mole ot NILC1(S) from the elements Na (g). H: (B) and Clh (g. EQUATION (3): Use the two following equations and Equations (1) and (2), sound previously, to calculate the enthalpy formation for NIH.CI(s). Apply Hess's Law so that the four equations add together to give Equation (3) abe of Given data Heo--19.29 kcal Y N2 (8) + H:(g)NH (aq) ju (g) +를C12(g) Heo HCl (aq) Equations to add together aHnn_-39.36 kcal 1) 2) objective of this experiment is to calculate the enthalpy of formation for NH CI(s). (Rem nder heat of formation is the ΔΗ for the formation of one mole of a compound from the elements Write the balanced chemical equation for the formation of 1 mole of NH CI(S) from the elements (, (8) and Cl2 (g). EQUATION (3): Use the two following formation for NH4CI(s). Apply Hess's Law so that the four equations add together to give Equation (3) abor Given data: equations and Equations (1) and (2), found previously, to calculate the enthalpy of ur equations add together to give Equation (3) abo 를 N2 (g)憬H2(g) H2O NH3 (aq) AHma-19.29 kcal X H20 Cl2 (g)-→ HCI (aq) ΔΗη,--39.36 kcal H2 (g) + Equations to add together: 1) 2) 3) 4)

Answer 1

19.29-33 36)+ (638)+(-3-33) 69.06 Kca!