Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(𝑔) + Cl₂(𝑔) ⇌ 2 NOCl(𝑔) At 700 K, the equilibrium constant 𝐾_𝑝 for this reaction is 0.26. For each of the following mixtures at this temperature, indicate whether the mixture is at equilibrium, or, if not, whether it needs to produce more products or reactants to reach equilibrium. (b) 𝑃_NO= 0.12atm, 𝑃_Cl2= 0.10atm, 𝑃_NOCl= 0.050atm

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Calculate the reaction quotient, Qp, using the formula: Qp = (P_NOCl)^2 / (P_NO)^2 * (P_Cl2).

Substitute the given partial pressures into the Qp expression: P_NO = 0.12 atm, P_Cl2 = 0.10 atm, P_NOCl = 0.050 atm.

Compare the calculated Qp value with the given equilibrium constant Kp = 0.26.

If Qp = Kp, the system is at equilibrium. If Qp < Kp, the reaction will proceed in the forward direction to produce more products. If Qp > Kp, the reaction will proceed in the reverse direction to produce more reactants.

Based on the comparison, determine whether the mixture is at equilibrium or if it needs to shift to reach equilibrium.

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Key Concepts

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

Equilibrium Constant (Kp)

The equilibrium constant, Kp, quantifies the ratio of the partial pressures of products to reactants at equilibrium for a given reaction. For the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g), Kp is calculated as (P_NOCl^2) / (P_NO^2 * P_Cl2). A Kp value of 0.26 indicates that at equilibrium, the concentration of products is relatively low compared to reactants, guiding predictions about the direction of the reaction.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by changes in concentration, pressure, or temperature, the system will adjust to counteract the disturbance and restore a new equilibrium. In this context, if the partial pressures of NO, Cl2, or NOCl are altered, the reaction will shift towards the side that reduces the effect of the change, either producing more products or reactants.

Reaction Quotient (Q)

The reaction quotient, Q, is calculated using the same formula as Kp but with the current partial pressures of the reactants and products. By comparing Q to Kp, one can determine the direction in which the reaction will proceed to reach equilibrium. If Q < Kp, the reaction will shift to the right (producing more products), while if Q > Kp, it will shift to the left (producing more reactants).

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Reaction Quotient Q

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For the equilibrium PH₃BCl₃(𝑠) ⇌ PH₃(𝑔) + BCl₃(𝑔) 𝐾_𝑝 = 0.052 at 60°C. (b) A closed 1.500-L vessel at 60°C is charged with 0.0500 g of BCl₃(𝑔); 3.00 g of solid PH₃BCl₃ is then added to the flask, and the system is allowed to equilibrate. What is the equilibrium concentration of PH₃?

Textbook Question

A 0.831-g sample of SO₃ is placed in a 1.00-L container and heated to 1100 K. The SO₃ decomposes to SO₂ and O₂: 2SO₃(𝑔) ⇌ 2 SO₂(𝑔) + O₂(𝑔) At equilibrium, the total pressure in the container is 1.300 atm. Find the values of 𝐾_𝑝 and 𝐾_𝑐 for this reaction at 1100 K.

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Textbook Question

At 900 °C, 𝐾_𝑐= 0.0108 for the reaction

CaCO₃(𝑠) ⇌ CaO(𝑠) + CO₂(𝑔)

A mixture of CaCO₃, CaO, and CO₂ is placed in a 10.0-L vessel at 900°C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium?

(a) 15.0 g CaCO3, 15.0 g CaO, and 4.25 g CO2

(b) 2.50 g CaCO3, 25.0 g CaO, and 5.66 g CO2

Textbook Question

The equilibrium constant constant 𝐾_𝑐 for C(𝑠) + CO₂(𝑔) ⇌ 2 CO(𝑔) is 1.9 at 1000 K and 0.133 at 298 K. (a) If excess C is allowed to react with 25.0 g of CO2 in a 3.00-L vessel at 1000 K, how many grams of CO are produced? (b) If excess C is allowed to react with 25.0 g of CO₂ in a 3.00-L vessel at 1000 K, how many grams of C are consumed?

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