Solid ammonium carbonate, (NH4)2CO3, decomposes to produce NH3 and CO2 gases and water vapor according to...
Solid ammonium carbonate, (NH4)2CO3, decomposes to produce NH3 and CO2 gases and water vapor according to the following equation:
(NH4)2CO3 (s) «2NH3 (g) + CO2 (g) + H2O (g)
A certain amount of solid ammonium carbonate, (NH4)2CO3, was placed in an evacuated and sealed 5,00-L flask and heated to 673 K. Some of the solid decomposed until equilibrium according to the above equation.
- Write an expression for the equilibrium constant kp for this reaction in terms of partial pressures,
- If the vapor pressure of water at equilibrium was 0.522 atm, (i) what were the equilibrium partial pressures of NH3 and CO2, respectively? (ii) What was the total gas pressure at equilibrium?
- Calculate the equilibrium constants kp and kc, respectively for the above equilibrium at 673 K.
- How many grams of (NH4)2CO3 had completely decomposed when equilibrium was established at the above temperature?
Homework Answers
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Solid ammonium carbonate, (NH4)2CO3, decomposes to produce
NH3 and CO2 gases and water vapor according
to...
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If 1.5g of ammonium carbamate is placed in a 1.50L flask and
some CO2 is added so that the partial pressure of CO2 at
equilibrium is 1.5atm, what is the partial pressure of NH3 when the
system comes at equilibrium at 25 degrees?
The final answer should be 0.0214barr or atm, please show your
work, thank you.
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CaCO3(s) = Cao (s)+CO2 (g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0 mol sample of CaCO3(s) is placed in a rigid 100. L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00 atm, while some CaCO3(s) remains in the vessel. a. Calculate...
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9. (10 pts) Solid ammonium carbamate decomposes to ammonia and carbon dioxide: N,H.CO2 (s) → 2 NH3(g) + CO2(g) At room temperature the total pressure of ammonia and carbon dioxide over ammonium carbonate is 0.116 atm, What is the equilibrium constant for the reaction?
If 1.5g of ammonium carbamate is placed in a 1.50L flask and
some CO2 is added so that the partial pressure of CO2 at
equilibrium is 1.5atm, what is the partial pressure of NH3 when the
system comes at equilibrium at 25 degrees?
The final answer should be 0.0214barr or atm, please show your
work, thank you.
Ammonium carbamate, NH4CO2NH2, dissociates according to the exothermic reaction: 4.62 × 10-4 at 25°C NH,co2NH2 (s) 2 NH2(g) + CO2(g) Kp
Ammonium carbamate,...
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