The following acid-base reaction occurs spontaneously in the gas phase: NH3(g) + HCl(g) = NH₂Cl(s) During an experiment, 14.00 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 x 10¹5, determine the partial pressures (in atm) of NH3 and HCI after the reaction reaches equilibrium. 1 4 7 +/- 2 5 8 atm 3 6 9 0 X C x 100

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9:10
1
4
7
+/-
Question 4 of 10
The following acid-base reaction
occurs spontaneously in the gas
phase:
NH3(g) + HCI(g) ⇒ NH₂Cl(s)
During an experiment, 14.00 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
x 10¹5, determine the partial
pressures (in atm) of NH3 and HCI
after the reaction reaches
equilibrium.
2
5
8
atm
3
60
9
O
Submit
Tap here or pull up for additional resources
XU
x 100
Transcribed Image Text:9:10 1 4 7 +/- Question 4 of 10 The following acid-base reaction occurs spontaneously in the gas phase: NH3(g) + HCI(g) ⇒ NH₂Cl(s) During an experiment, 14.00 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 x 10¹5, determine the partial pressures (in atm) of NH3 and HCI after the reaction reaches equilibrium. 2 5 8 atm 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
Expert Solution
Step 1

Given acid-base reaction

NH3(g)+HCl(g)NH4Cl(s)

Equilibrium constant = K=8.9×1015

At equilibrium PNH3=?

At equilibrium PHCl=?

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