Calculate K c for each reaction. a. I 2 (g) ⇌ 2I(g) K p = 6.26⨉10 -22 (at 298K)

Hello everyone today. We are being given the following reaction and a following K. P value at a specific temperature and asked to calculate K. C. First thing we wanna do is recall the equation that we want to use and that is K P. Is equal to K. C. Times the gas constant times the temperature raised to the difference in moles rearranging. This equation gives us Casey is equal to K. P over gas constant times the temperature. And then we have that difference in moles. So on the product side we have two moles of gas represented by the coefficient. So we say two minus how many moles of gas we have on the reactant side. We have two of you know and one of B R two. So we have three moles of gas on the reactant two minus three where they gonna plug in. Our values were going to say That RKP value is 2.4. The gas constant is 0.08-1 And we have our temperature but it has to be in Kelvin. So we're going to add 73.15-100. And that gives us 373.15 Kelvin plug that in. And then of course our 2 -3 in the exponent This is going to give us a final value. Final KC value of 73.49. I hope this helped. And until next time

Ch.15 - Chemical Equilibrium

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Tro 4th Edition

Ch.15 - Chemical Equilibrium

Problem 31a

Chapter 15, Problem 31a

Calculate K_c for each reaction. a. I₂(g) ⇌ 2I(g) K_p = 6.26⨉10^-22 (at 298K)

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Identify the given values and the required conversion: You are given the equilibrium constant in terms of pressure (Kp) and need to calculate the equilibrium constant in terms of concentration (Kc) for the reaction at a specific temperature (298K).

Write down the balanced chemical equation for the reaction: I2(g) ⇌ 2I(g).

Use the relationship between Kp and Kc, which is Kp = Kc(RT)^Δn, where R is the gas constant (0.0821 L atm K^-1 mol^-1), T is the temperature in Kelvin, and Δn is the change in moles of gas (moles of products - moles of reactants).

Calculate Δn for the reaction: Δn = 2 (moles of I) - 1 (moles of I2) = 1.

Substitute the values of Kp, R, T, and Δn into the formula to solve for Kc: Kc = Kp / (RT)^Δn.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kc and Kp)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.

Relationship Between Kc and Kp

Kc and Kp are related through the ideal gas law and the stoichiometry of the reaction. For reactions involving gases, the conversion between Kc and Kp depends on the difference in the number of moles of gaseous products and reactants. This relationship allows for the calculation of one constant if the other is known, provided the temperature remains constant.

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. In the given reaction, I2(g) ⇌ 2I(g), the stoichiometry indicates that one mole of iodine gas dissociates into two moles of iodine atoms. This stoichiometric ratio is crucial for calculating Kc from Kp, as it directly influences the value of Δn in the Kp-Kc relationship.

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Textbook Question

This reaction has an equilibrium constant of K_p = 2.2⨉10⁶ at 298 K. 2 COF₂(g) ⇌ CO₂(g) + CF₄(g) Calculate K_p for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 6 COF₂(g) ⇌ 3 CO₂(g) + 3 CF₄(g)