The final pressure of the system is equal to 0.960 atm after the reaction is complete.
The state of an ideal gas is described in terms of its pressure, volume, and temperature. The ideal gas law can be represented in the terms of the product of the volume and pressure is equal to the multiplication of the absolute temperature, moles of gas, and the universal gas constant.
An ideal gas of mathematical equation can be written as follows:
PV = nRT
The balanced chemical equation of ammonia and HCl:
[tex]NH_3 (g) + HCl (g) \longrightarrow NH_4Cl(s)[/tex]
Given the mass of ammonia, m = 5.00 g
The number of moles of ammonia = 5/17 = 0.294 mol
The number of moles of HCl, n = PV/RT
[tex]n = \frac{1.68 atm\times 2L}{0.082 \times 298 K}[/tex]
n = 0.137 mol
The number of moles of NH₃ did not react, n = 0.294 - 0.137 = 0.157 mol
The final pressure of the system after the reaction is complete:
[tex]{\displaystyle {P = \frac{nRT}{V}[/tex]
[tex]{\displaystyle {P = \frac{0.157 \times 0.082 \times 298}{4}[/tex]
P = 0.960 atm
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Your question was incomplete, but most probably the complete question was,
Ammonia and hydrogen chloride react to form solid ammonium chloride: Two 2.00-L flasks at 25 degrees C are connected by a valve, as shown in the drawing. One flask contains 5.00 g ammonia, and the other contains HCl(g) at 1.68 atm. When the valve is opened, the gases react until one is completely consumed. What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.)
