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NH4CO2NH2(s) equilibrium reaction arrow 2 NH3(g) + CO2(g) Ammonium carbamate decomposes according to the equation above. At 40°C, an equilibrium mixture for this reaction contains 0.0640 atm CO2 and 0.370 atm NH3. What is the value of the equilibrium constant Kp for the reaction?

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anfabba15

Answer:

Kp = 8.76×10⁻³

Explanation:

We determine the carbamate decomposition in equilibrium:

NH₄CO₂NH₂ (s) ⇄ 2NH₃(g) + CO₂(g)

Let's build the expression for Kp

Kp = (Partial pressure NH₃)² . Partial pressure CO₂

We do not consider, the carbamate because it is solid and we only need the partial pressure from gases

Kp = (0.370atm)² . 0.0640 atm

Kp = 8.76×10⁻³

Remember Kp does not carry units

 

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