I do rate the answer, so please answer it seriously!!! Ammonia and hydrogen chlo

Question

I do rate the answer, so please answer it seriously!!!

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 NH3(g), and the other contains HC a1.68 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 2.00 L 25°C HCl(g) 1.68 atm 2.00 25°C

Explanation / Answer

Moles of ammonia= mass/molar mass=5/17=0.29

Moles of HCL= PV/RT

=1.68*2/(0.0821*298)=0.14

NH3(g)+HCl(g)----------àNH4Cl(s)

Theoretical molar ratio of NH3:HCl=1:1

Actual molar ratio of NH3:HCl =0.29:0.14

Limiting reactant is HCl.

Moles of NH3 is excess.

Moles of NH4Cl formed from limiting reactant=0.14

mass of NH4Cl formed= 0.14*53.5 =7.5 gm

Moles of NH3 remaining = 0.29-0.14=0.15

n= 0.15   V=volume of two tanks= 2+2= 4L

T=25+273=298K

P= nRT/V= 0.15*0.0821*298/4

=0.92 atm

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