The following acid-base reaction occurs spontaneously in the gas phase: NH₃(g) + HCl(g) ⇌ NH₄Cl(s) During an experiment, 18.00 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
The following acid-base reaction occurs spontaneously in the gas phase: NH₃(g) + HCl(g) ⇌ NH₄Cl(s) During an experiment, 18.00 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.
The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of product to that of the reactants raised to power their specific stoichiometric coefficients in the balanced chemical equation. The value of the equilibrium constant does not alter by the addition of the catalyst in the chemical reaction.
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