Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chl

Question

Ammonia, NH3(g), and hydrogen chloride, HCl(g), react to form solid ammonium chloride, NH4Cl(s): NH3(g)+HCl(g)NH4Cl(s)
Two 1.50 L flasks at 30.0 C are connected by a stopcock, as shown in the drawing

One flask contains 5.20gNH3(g), and the other contains 5.00 g  HCl(g). When the stopcock is opened, the gases react until one is completely consumed.

1. What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.) (atm*)

2. What mass of ammonium chloride will be formed? (g)

Explanation / Answer

the reaction is NH3(g) + HCl (g) ---->NH4Cl(g)

moles : mass/molar mass

moles : NH3= 5.2/17 =0.3058, HCl = 5/36.5=0.14

molar ratio of NH3: HCl ( theoretical) =1:1, actutla ratio = 0.3058:0.14= 2.2 :1

HCl is excess, mole o NH3L remaining after reaction = 0.3058-0.14= 0.1658

T= 30+273= 303 K, V= 1.5L, P= nRT/V= 0.1658* 0.0821*303/1.5 =2.75 atm

mole og NH4Cl formed= 0.14 mass of NH4Cl = moles* molar mass = 0.14*53.5 =7.5 gm

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