Solid ammonium carbamate dissociated according to the given reactionNH2COONH4(s) 2NH3(g) + CO2(g)If total pressure at equilibrium is 6 atm then Kp will
Question
Solid ammonium carbamate dissociated according to the given reactionNH2COONH4(s) 2NH3(g) + CO2(g)If total pressure at equilibrium is 6 atm then Kp will
Solution
The given reaction is:
NH2COONH4(s) ⇌ 2NH3(g) + CO2(g)
According to the problem, the total pressure at equilibrium is 6 atm.
Since the reaction involves the dissociation of a solid into gases, we can assume that all of this pressure is due to the gases NH3 and CO2.
The stoichiometry of the reaction tells us that for every mole of NH2COONH4 that dissociates, 2 moles of NH3 and 1 mole of CO2 are produced. Therefore, the partial pressures of NH3 and CO2 at equilibrium are in the ratio 2:1.
Let's denote the partial pressure of CO2 as P(CO2) and the partial pressure of NH3 as P(NH3).
Since the total pressure is 6 atm, we can write:
P(CO2) + P(NH3) = 6 atm
And since the partial pressures are in the ratio 2:1, we can write:
P(NH3) = 2 * P(CO2)
Substituting the second equation into the first, we get:
P(CO2) + 2 * P(CO2) = 6 atm
Solving for P(CO2), we find:
P(CO2) = 2 atm
Substituting this back into the equation P(NH3) = 2 * P(CO2), we find:
P(NH3) = 4 atm
The expression for the equilibrium constant Kp for the reaction is:
Kp = [P(NH3)]^2 * [P(CO2)]
Substituting the values we found, we get:
Kp = (4 atm)^2 * (2 atm) = 32
So, the Kp for the reaction is 32.
Similar Questions
Solid ammonium carbmate (NH2CO2NH4) dissociates completely into ammoniaand carbon dioxide when it evaporates:2 2 4 3 2NH CO NH s 2 NH g CO gAt 298 K, the total pressure of the gases in equilibrium with the solid is 3 atm. Calcu-late the value ofequilibrium constant Kp
A mixture containing C5H6, HCl, Cl2, and C5H8, all at an initial partial pressure of 4.74 atm, is allowed to achieve equilibrium according to the equation below. At equilibrium, the partial pressure of C5H8 is observed to have decreased by 0.82 atm. Determine Kp for this chemical equilibrium. Report your answer to 3 significant figures in scientific notation.C5H6(g) + 2HCl(g) ⇌ Cl2(g) + C5H8(g)
In the equilibrium system N2(g) + 3H2(g) → 2NH3(g)Kc = 2.0 mol-2dm6 at 620 K. What is the value of Kp at this temperature.
OCl2(g) ⇄ CO(g) + Cl2(g)COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previouslyevacuated flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K
Two moles of ammonia is introducedi in an evacuated 500 ml vessel at high temperature. The decomposition reaction is : 2NH3 ->N2 +3H2 at the equillibrium NH3 becomes 1 mole then the 'K' would be:
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.