(288) ( 2. (20 points) Ammonia and hydrogen chloride react to form solid ammoniu
ID: 558015 • Letter: #
Question
(288) ( 2. (20 points) Ammonia and hydrogen chloride react to form solid ammonium chloride: NH3(g) + HCl(g) NH4Cl(s) Two 2.00-L flasks at 25°C are connected by a valve, as shown in the drawing. One flask contains 5.00 g NHs(g), and the other contains HCl(g) at 1.68 atm. When the valve is opened, the gases react until one is completely consumed. (a) What mass of ammonium chloride will be formed? (b) What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.) NH3(g) 5.00 g 2.00 L 25°C HCl(g) 1.68 atm 2.00 L 25°CExplanation / Answer
a)
mol of NH3 = mass/MW = 5/17 = 0.29411
mol of HCl = PV/(RT) = (1.68*2)/(0.082*298) = 0.13750
ratio is 1:1 so HCl limits reaction
mol of NH4Cl --> mol of HCl = 0.13750 mol of NH4Cl
mass =mol*MW = 0.13750*53.4915 = 7.355 g of NH4Cl
find final P:
mol left = 0.29411-0.13750 = 0.15661
mol prouced = 0.13750
total mol = 0.13750 +0.15661 = 0.29411
then
PV = nRT
V = V1+V2 =2+2 = 4
T = 298K,
P = nRT/V = (0.29411)(0.082)(298)/(4) = 1.7967 atm
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