Consider the reaction: Br2(g)+Cl2(g) ⇌2 BrCl(g) Kp=1.11 ×10^-4 at 150 K A reaction mixture initi

step 1 We have the following reaction. A reaction mixture inexually contains a BR2 partial pressure of

Consider the reaction: Br2(g)+Cl2(g) ⇌2 BrCl(g) Kp=1.11...

Consider the reaction: $$\mathrm{Br}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{BrCl}(g) K_{\mathrm{p}}=1.11 \times 10^{-4} \mathrm{at} 150 \mathrm{K}$$ A reaction mixture initially contains a $\mathrm{Br}_{2}$ partial pressure of 755 torr and a $\mathrm{Cl}_{2}$ partial pressure of 735 torr at 150 $\mathrm{K}$ . Calculate the equilibrium partial pressure of BrCl.

Consider the reaction:
$$\mathrm{Br}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{BrCl}(g) K_{\mathrm{p}}=1.11 \times 10^{-4} \mathrm{at} 150 \mathrm{K}$$
A reaction mixture initially contains a $\mathrm{Br}_{2}$ partial pressure of 755 torr and a $\mathrm{Cl}_{2}$ partial pressure of 735 torr at 150 $\mathrm{K}$ . Calculate the equilibrium partial pressure of BrCl.

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, leading to constant concentrations or partial pressures of all species involved. At equilibrium, the system has reached a balance and the macroscopic properties remain unchanged over time, although microscopic processes continue to occur.

Equilibrium Constant (Kp)

The equilibrium constant, specifically Kp for reactions involving gases, is a dimensionless number that quantifies the ratio of product partial pressures to reactant partial pressures at equilibrium, each raised to the power of their stoichiometric coefficients. It provides a measure of the extent to which a reaction proceeds and is specific to a given temperature.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction as expressed by the balanced chemical equation. It is used to determine how changes in the amount or partial pressure of one species affect other species, ensuring that the proportions dictated by the reaction coefficients are maintained.

ICE Table Method

The ICE (Initial, Change, Equilibrium) table is a systematic approach used to organize and calculate the concentrations or partial pressures of reactants and products as a system approaches equilibrium. By accounting for the initial conditions, the changes that occur during the reaction, and the resulting equilibrium state, it simplifies solving equilibrium problems.

Gaseous Equilibrium Partial Pressures

In reactions involving gases, the partial pressures of each gas can be used in place of concentrations to describe the state of the system at equilibrium. The behavior of these gases is typically described by the ideal gas law, and their partial pressures are directly related to the mole fractions and total pressure in the system.

Transcript

00:01 We have the following reaction.

00:04 A reaction mixture inexually contains a br2 partial pressure of 754.

00:10 So we have the partial pressure of br2 is equal to 755 tor.

00:24 And we also have that the initial pressure of co2 is equal to 735.

00:36 Well, recall that when we're working with kp values, or just concentrations in terms of partial pressures, we need to convert them to atm.

00:46 So let's convert them to atm.

00:47 We're gonna divide by 160 tor, which is equal to 1 atm.

01:01 Well, that gives me, let me take out the calculator, 755 divided by 760, that gives me 0 .993 atm and 0 .96m.

01:21 Okay, so let's draw out our ice table.

01:27 So we have our pressure of br2, our pressure of cl2, and our pressure of brcl2, and our pressure of brcl.

01:37 Well, we know the initial, which we're at these two, is .993 and 0 .967.

01:43 Okay, let's look back our question.

01:49 We're asked to calculate the equilibrium partial pressure of br, cl.

01:53 So we're looking for this term right here.

01:57 Okay, so since it wasn't stated anything about the partial pressure of brcl, we know that its initial is zero.

02:06 Now, what shall we do? let's check which direction our reaction is going.

02:15 We know that qc is equal to zero by inspection since there is no products in the beginning.

02:23 So we know that qc is less than kp, so our reaction is actually going to the right.

02:28 Because of this, our products have a positive change and our reactants have a negative change.

02:38 And if you recall since drcl has a 2 here, we need to multiply by 2 and the remaining are 1, so that's fine...

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