Calculate K p for each reaction. a. N 2 O 4 (g) ⇌ 2 NO 2 (g) K c = 5.9⨉10 -3 (at 298 K)

Hello everyone today, we have been given a following reaction with the K. C value at a specific temperature and asked to determine the value of K. P. Well, first we want to write the equation that we're gonna be using and that is K. P. What we want to find is equal to K. C. Times the gas constant times the temperature. And we're going to raise that to the difference in in or the difference in moles which represented by delta in. We have our k. c value which is 6.9 six times 10 to the -5. R. Gas Constant is 0.08 - one. And our temperature while in C we must convert to Kelvin by adding to 73 0.15. That gives us 333.15 Kelvin. So we're gonna write that here and then we have the difference in moles of gas and that's going to be from products to reactant. So on our product side we have one mole of ph three and one mole of BCL three which gives us two moles total. We're gonna write two minus And then we have zero moles on of gas on the reactant side. So we're going to say -0 -0 0 Calculations will yield us a final answer of 0.05, two. I hope this helped. And until next time

Ch.16 - Chemical Equilibrium

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Tro 5th Edition

Ch.16 - Chemical Equilibrium

Problem 32a

Chapter 16, Problem 32a

Calculate K_p for each reaction. a. N₂O₄(g) ⇌ 2 NO₂(g) K_c = 5.9⨉10^-3 (at 298 K)

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Identify the balanced chemical equation for the reaction: N2O4(g) ⇌ 2NO2(g).

Understand the relationship between Kc and Kp: Kp = Kc(RT)^{\Delta n}, where R is the gas constant (0.0821 L atm K^{-1} mol^{-1}), T is the temperature in Kelvin, and \Delta n is the change in moles of gas (moles of products - moles of reactants).

Calculate \Delta n for the reaction: \Delta n = 2 - 1 = 1.

Substitute the values into the equation: Kp = (5.9 \times 10^{-3}) \times (0.0821 \times 298)^1.

Simplify the expression to find Kp.

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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 (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Kp, on the other hand, is the equilibrium constant expressed in terms of partial pressures of gases. 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.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of Kp, it refers to the pressure of each gas in the reaction when it is at equilibrium. The total pressure of the gas mixture is the sum of the partial pressures of all the gases present, and understanding this concept is crucial for calculating Kp from Kc.

Change in Moles of Gas (Δn)

Δn is defined as the difference between the number of moles of gaseous products and the number of moles of gaseous reactants in a balanced chemical equation. This value is essential for converting Kc to Kp, as it indicates how the number of gas molecules changes during the reaction. A positive Δn suggests an increase in gas moles, while a negative Δn indicates a decrease, affecting the relationship between Kc and Kp.