At 25°C, Kp = 2.910−3 for the following reaction.
NH4OCONH2(s) 2 NH3(g) + CO2(g)
In an experiment carried out at 25°C, a certain amount of NH4OCONH2 is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.
I can't tell what the value of Kp is. I will assume you meant it to be 2.91E-3. BTW, you need to learn where the arrow key is too. The arrow tells us where the reactants stop and the products begin.
......NH4OCONH2(s) ==> 2NH3 + CO2
I.......solid...........0.......0
C.......solid...........2x.......x
E.......solid...........2x......x
Kp = p^2NH3*pCO2
Kp = (2x)^2(x)
Solve for x, 2x, and add the two pressures to find the total pressure.
312 / 5000
Resultados de traducción
At 25 ∘C, Kp = 2.9 × 10−3 for the reaction
NH4OCONH2 (s) ↽ −− ⇀2NH3 (g) + CO2 (g)
In an experiment at 25 ∘C, a certain amount of NH4OCONH2 (s) is placed in an empty rigid container and allowed to reach equilibrium.
Calculate the partial pressures of each gas and the total pressure in the container at equilibrium.
To calculate the total pressure in the container at equilibrium, we need to use the equilibrium constant (Kp) and the stoichiometry of the reaction.
First, let's write the balanced chemical equation for the reaction:
NH4OCONH2(s) 2 NH3(g) + CO2(g)
According to the equation, for every mole of NH4OCONH2 that reacts, 2 moles of NH3 and 1 mole of CO2 are formed.
Since Kp is given, Kp = P(NH3)^2 * P(CO2) / P(NH4OCONH2)
Given that Kp = 2.910^-3, we can express this equation as:
2.910^-3 = (P(NH3))^2 * P(CO2) / P(NH4OCONH2)
To find the total pressure at equilibrium, we need to find the partial pressures of NH3 and CO2.
Let's assume that x is the amount of NH4OCONH2 that reacted, then 2x will be the amount of NH3 and x will be the amount of CO2 formed.
The volume of the container is assumed to be constant and the number of moles of gas remains constant, so we can express the partial pressures in terms of x:
P(NH3) = 2x
P(CO2) = x
P(NH4OCONH2) = (initial number of moles of NH4OCONH2 - x)
Since the container is evacuated before the reaction, the initial number of moles of NH4OCONH2 is equal to the number of moles of NH4OCONH2 placed in the container.
Finally, we substitute these values into the Kp expression and solve for x:
2.910^-3 = (2x)^2 * x / (initial number of moles of NH4OCONH2 - x)
After solving this equation, we can find the value of x. Then, we substitute this value into our partial pressure expressions to find the partial pressures of NH3 and CO2.
Lastly, we calculate the total pressure by adding the partial pressures of NH3 and CO2 and any other gases present in the container.
To calculate the total pressure in the container at equilibrium, we need to use the equilibrium constant (Kp) and partial pressures of the gases involved in the reaction.
In this case, the equilibrium constant (Kp) is given as 2.910−3.
The balanced equation for the reaction is:
NH4OCONH2(s) → 2 NH3(g) + CO2(g)
Since NH4OCONH2 is a solid, its concentration does not change and does not affect the equilibrium constant. Therefore, the partial pressures of NH3 and CO2 will determine the total pressure in the container.
Let's assume that the initial moles of NH4OCONH2 placed in the container is "x" moles. Since 1 mole of NH4OCONH2 produces 2 moles of NH3 and 1 mole of CO2, at equilibrium, we will have "2x" moles of NH3 and "x" moles of CO2.
The partial pressure for NH3 (P(NH3)) can be calculated using the ideal gas law:
P(NH3) = (n(NH3) * R * T) / V
where n(NH3) is the number of moles of NH3, R is the ideal gas constant (0.0821 L atm/(mol K)), T is the temperature in Kelvin (25°C = 298K), and V is the volume in liters.
Similarly, the partial pressure for CO2 (P(CO2)) can be calculated using the same formula:
P(CO2) = (n(CO2) * R * T) / V
where n(CO2) is the number of moles of CO2.
Now, we know that the molar ratio of NH3 to CO2 is 2:1, which means that for every mole of CO2, we will have 2 moles of NH3. So, n(CO2) = x, and n(NH3) = 2x.
Substituting these values into the partial pressure formulas, we get:
P(NH3) = (2x * 0.0821 * 298) / V
P(CO2) = (x * 0.0821 * 298) / V
Since the total pressure (P(total)) in the container is the sum of the partial pressures of NH3 and CO2, we have:
P(total) = P(NH3) + P(CO2)
P(total) = (2x * 0.0821 * 298) / V + (x * 0.0821 * 298) / V
Simplifying the equation:
P(total) = (2 * 0.0821 * 298 * x + 0.0821 * 298 * x) / V
P(total) = (0.1642 * 298 * x + 0.0821 * 298 * x) / V
P(total) = (0.2463 * 298 * x) / V
Finally, substituting the value of x into the equation gives us the total pressure in the container at equilibrium.