Question

NH,(8) + HCl(g) NH,Cl(s) A 6.55 g sample of NH, gas and a 6.55 g sample of HCl gas are mixed in a 1.50 L flask at 25°C. Identify the limiting reagent. HCI ONH,CI Ο ΝΗ, How many grams of NH CI will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH, CI produced by the reaction.

Answer 1

Answer

Balanced chemical Equation moles of NH3 left = 3.50 g 17g molt NH3 Lg & Hi (g - Nhyll & = 0.205 mol using Idel Gas equation (to calculate pressure) Molar molar mass of with a 17g mot mass of Hel = 36.5 gone Pr - MRT 36.5 g Hel reacts completely with NH₂ - 17 P = MRT Thus, 16:53 g Hd will react completely with Nath - 17g XG-55g - 36.57 Latm k'mol (298k) = 10.205 mol - (0.062 1.50 h - 3-050 9 is 3.339 atm 2 3.34 abon Tuus, Hell is present in completely With available the limiting lesser amount reacting with in excess of Reagent (The reagent than required for the other reagents) Limiting leegent decides the amount of product - molar mass of NHyll= 53.5 gmol 36.5 g Hill reacts completely to form till = 53.5 gms 6.35g He will react completely to form tyle - 53.5 X 6.5 - 36.5 g - = 9.600 g Armant of Nu remains unreacted = 6.55 -3.05g