Question

A 10.0L reaction flask contains ammonia at 0.452atm, and 22°C. When 155mL of hydrogen chloride gas, measured at 7.50atm and 271K, is introduced to the flask, the two gases react to produce solid ammonium chloride. Determine the pressure inside the flask after the reaction is complete and the temperature has returned to 22°C. Ignore the volume of the solid produced.

Answer 1

From Ideal Grab équation Pi=nRT n2 PV RT (MMH ) = (0.452 atm) (10L) (0.0821 Latm/K moi) (22 +2784 No of moles of Ammonia MH, = 2 No of moles of 0.1866 moles 0-186 Hel (MH) = (7.50 atm) (10L) (0.0821 Latmik.mei) (271k) MHG = 3.37 moles NH + HCl -> NH4Class (8 9) Imole (mole 0.186 from the above equation Imole of NH3 reacts with Imole of Hol. => 0.186 moles of Nity reacts with our moles of HCl i Amount of Hel gas remained (un reacted) = (3.370 0186) moles = 3:1844 moles after the reaction .. pressure of the gas (HCl) P = MRI

- (31184 mol) (0:0821 Latm.mot k') (295k) - 10L P = 7.7 atm . pressure of the gas in the Flalk 2 7.7 atm.