Question

The following acid-base reaction occurs spontaneously in the gas phase: NH₃(g) + HCl(g) ⇌ NH₄Cl(s) During an experiment, 10. 00 g of solid NH₄Cl was added to a 500. 0 mL flask at 25. 0°C. The equilibrium constant for this reaction at this temperature is 8. 9 × 10¹⁵, determine the partial pressures (in atm) of NH₃ and HCl after the reaction reaches equilibrium

Answer 1

The partial pressures (in atm) of NH₃ and HCl after the reaction reaches equilibrium is mathematically given as

• PH3=1.06*10^{-8}atm
• PHCl=1.06*10^{-8}atm

What is the partial pressures (in atm) of NH₃ and HCl after the reaction reaches equilibrium?

Question Parameter(s):

Generally, the equation for the Chemical Reaction  is mathematically given as

HCl(g) ⇌ NH₄Cl(s)

Therefore

$Keq=\frac{1}{PH3*PHC}$

PH3*PHCl=1.23*10^16

Therefore

P^2=1.23*10^{-16}

P=1.06*10^{-8}

In conclusion,

PH3=1.06*10^{-8}atm

PHCl=1.06*10^{-8}atm

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