1
Question
Solid ammonium carbamate, NH4CO2NH2(s), dissociates into ammonia and carbon dioxide, when it evaporates as shown by: NH4CO2NH2(s)⇌2NH3(g)+CO2(g). At 25oC, the total pressure of the gases in equilibrium with the solid is 0.116 atm. If 0.1 atm of CO2 is introduced after equilibrium is reached, then:
Solid ammonium carbamate, NH4CO2NH2(s), dissociates into ammonia and carbon dioxide, when it evaporates as shown by: NH4CO2NH2(s)⇌2NH3(g)+CO2(g). At 25oC, the total pressure of the gases in equilibrium with the solid is 0.116 atm. If 0.1 atm of CO2 is introduced after equilibrium is reached, then:
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Solution
The correct options are
A the pressure of NH3 will decrease due to addition of CO2
D the final pressure of CO2 will be more than 0.1 atm
The total pressure at equilibrium will be only due to ammonia and carbon dioxide. Solid ammonium carbamate does not contribute any pressure. There are two moles of ammonia and 1 mole of carbon dioxide.
Thus, 2p+1p=0.116⟹p=0.0386= Pressure due to carbon dioxide⟹2p=0.0774= Pressure due to ammonia
When carbon dioxide is added, it will react with ammonia and the equilibrium will shift in the reverse direction. This will decrease the pressure of ammonia.
Hence, option C is correct and option D is incorrect.
When 0.1 atm of carbon dioxide is added, the equilibrium pressures will be 0.077−2x atm and 0.1386−x atm.
0.077−2x cannot be less than zero. Hence x cannot be greater than 0.0385.
Hence, 0.1386−x cannot be less than 0.1.
Thus, the final pressure of carbon dioxide will be more than 0.1 atm.
A the pressure of NH3 will decrease due to addition of CO2
D the final pressure of CO2 will be more than 0.1 atm
The total pressure at equilibrium will be only due to ammonia and carbon dioxide. Solid ammonium carbamate does not contribute any pressure. There are two moles of ammonia and 1 mole of carbon dioxide.
Thus, 2p+1p=0.116
⟹p=0.0386= Pressure due to carbon dioxide
⟹2p=0.0774= Pressure due to ammonia
When carbon dioxide is added, it will react with ammonia and the equilibrium will shift in the reverse direction. This will decrease the pressure of ammonia.
Hence, option C is correct and option D is incorrect.
When 0.1 atm of carbon dioxide is added, the equilibrium pressures will be 0.077−2x atm and 0.1386−x atm.
0.077−2x cannot be less than zero. Hence x cannot be greater than 0.0385.
Hence, 0.1386−x cannot be less than 0.1.
0.077−2x cannot be less than zero. Hence x cannot be greater than 0.0385.
Hence, 0.1386−x cannot be less than 0.1.
Thus, the final pressure of carbon dioxide will be more than 0.1 atm.
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