You place 0.0300 mol of pure SO3 in an 8.00-L flask at 1150 K. At equilibrium, 0.0058 mol of O2

step 1 Okay, so in this question, we have this chemical equation. We have the volume as 8 liters, and w

You place 0.0300 mol of pure SO3 in an 8.00-L flask at 1150...

You place 0.0300 mol of pure $\mathrm{SO}_{3}$ in an $8.00-\mathrm{L}$ flask at $1150 \mathrm{K}$. At equilibrium, 0.0058 mol of $\mathrm{O}_{2}$ has been formed. Calculate $K_{c}$ for the reaction at $1150 \mathrm{K}$ $$ 2 \mathrm{sO}_{3}(\mathrm{g}) \rightleftharpoons 2 \mathrm{sO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) $$

You place 0.0300 mol of pure $\mathrm{SO}_{3}$ in an $8.00-\mathrm{L}$ flask at $1150 \mathrm{K}$. At equilibrium, 0.0058 mol of $\mathrm{O}_{2}$ has been formed. Calculate $K_{c}$ for the reaction at $1150 \mathrm{K}$
$$
2 \mathrm{sO}_{3}(\mathrm{g}) \rightleftharpoons 2 \mathrm{sO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})
$$

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in which the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products over time. It is a dynamic balance where the reaction continues to occur without any net change in the composition of the system.

Equilibrium Constant (Kc)

The equilibrium constant, denoted as Kc, is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its stoichiometric coefficient as indicated by the balanced chemical equation. It provides insight into the extent of a reaction and is temperature-dependent.

ICE Table Method

The ICE table (Initial, Change, Equilibrium) is a systematic tool used to organize the initial concentrations, the changes that occur as the reaction approaches equilibrium, and the final equilibrium concentrations. This method is especially useful for solving equilibrium problems and calculating the equilibrium constant.

Reaction Stoichiometry

Reaction stoichiometry involves using the mole ratios indicated by a balanced chemical equation to relate the amounts of reactants and products. It is essential for determining how changes in the concentration or quantity of one species affect the others in the system.

Molarity and Concentration Calculations

Molarity is the concentration of a solution expressed as moles of solute per liter of solution. In equilibrium problems, converting the number of moles into molar concentrations by dividing by the volume of the container is a crucial step for accurately applying the equilibrium constant expression.

Transcript

00:01 Okay, so in this question, we have this chemical equation.

00:04 We have the volume as 8 liters, and we started off with 0 .03 modes of s .03, and at equilibrium, we have 0 .058 modes of oxygen.

00:17 So the first thing that we should do is we just convert these moles into molarity.

00:22 So we have, for s .o3, the concentration is equal to 0 .03 modes divided by 8 .3 .5.

00:33 Liters and we should get 3 .75 times 10 to the negative 3 as a molarity and then for oxygen so this con this mole is at equilibrium right so equilibrium so equilibrium equilibrium is 4 .02 is 0 .058 moles over 8 liters which is 7 .058 meters which is 7 .0.

01:09 2 .5 times 10 to the negative 4 as a malaria.

01:15 Now they want us to calculate the concentration, no, they want us to calculate kc for the reaction, right? so in order to do that, we need to set up an ice box.

01:27 So we have i, which is the initial concentration, c, which is the change in concentration, and e, which is the concentration at equilibrium.

01:36 So let me erase this.

01:39 Okay, so we know that the equilibrium concentration of 02 is 7 .25 times 10 to the negative 4.

01:49 And we know that the initial concentration of s .o3 is 3 .75 times 10 to the negative 3.

01:58 Right.

02:00 And we also know that the initial concentration of s .o2 and o2 are zero, right? because at time it goes zero, this s .o3 hasn't been turned into s .o .2 or o2.

02:11 Yet...

Please give Ace some feedback