Welcome to the article At 313 K this reaction has a tex K c tex value of 0 0689 X g 2Y g rightleftharpoons 2Z g Calculate tex K. On this page, you will learn the essential and logical steps to better understand the topic being discussed. We hope the information provided helps you gain valuable insights and is easy to follow. Let’s begin the discussion!
Answer :
You can substitute the given temperature, 313 K, into the equation along with the value of R to calculate the Kp value.
The question asks us to calculate the Kp value for the given reaction at 313 K. The reaction is represented as:
x(g) + 2y(g) ↔ 2z(g)
We are given the Kc value, which is 0.0689 at 313 K. Kc is the equilibrium constant expressed in terms of concentrations. In order to calculate Kp, the equilibrium constant expressed in terms of partial pressures, we can use the ideal gas law.
The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
To calculate Kp, we need to relate the partial pressures of the gases to their concentrations. Since the reaction involves the gases x, y, and z, we can assume that the gases behave ideally.
Let's assume that the initial partial pressures of x, y, and z are Px0, Py0, and Pz0 respectively.
At equilibrium, the partial pressures will be Px, Py, and Pz.
Using the stoichiometry of the reaction, we can write the equilibrium expression in terms of partial pressures:
Kp = (Pz)^2 / (Px * Py^2)
To find Kp, we need to determine the relationship between concentrations and partial pressures. We can use the ideal gas law to relate the number of moles and partial pressures:
P = (n/V) * RT
Since the volume and temperature are constant, we can rewrite the equation as:
P = (n/V) * R * T
Since the moles and volume are constant, the ratio of partial pressures is equal to the ratio of concentrations:
(Px / Py^2) = (Cx / Cy^2)
Therefore, we can rewrite the equilibrium expression in terms of concentrations:
Kc = (Cz)^2 / (Cx * Cy^2)
Since Kp and Kc are related by the equation:
Kp = Kc * (RT)^∆n
Where ∆n is the difference in the number of moles of gaseous products and gaseous reactants.
In this case, ∆n = (2-1-2) = -1.
Substituting the values into the equation, we get:
Kp = Kc * (RT)^-1
Kp = 0.0689 * (R * T)^-1
Kp = 0.0689 / (R * T)
Where R is the ideal gas constant and T is the temperature in Kelvin.
Please note that the ideal gas constant R is 0.0821 L·atm/(mol·K).
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