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Diagram (a) shows the reaction $\mathrm{A}_{2}(g)+$ $\mathrm{B}_{2}(g) \rightleftharpoons 2 \mathrm{AB}(g)$ at equilibrium at a certain temperature, where the blue spheres represent $A$ and the yellow spheres represent B. If each sphere represents 0.020 mole and the volume of the container is 1.0 L, calculate the concentration of each species when the reaction in (b) reaches equilibrium.

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A. $$\begin{array}{l}{\left[\mathrm{A}_{2}\right]=0.040 M} \\{\left[\mathrm{B}_{2}\right]=0.040 M} \\{[\mathrm{AB}]=0.020 M}\end{array}$$B. $$\begin{array}{l}{\left[\mathrm{A}_{2}\right]=0.040 \mathrm{M}} \\{\left[\mathrm{B}_{2}\right]=0.040 \mathrm{M}} \\{[\mathrm{AB}]=0.020 \mathrm{M}}\end{array}$$

Chemistry 102

Chapter 14

Chemical Equilibrium

Brown University

University of Toronto

Lectures

10:03

In thermodynamics, a state of thermodynamic equilibrium is a state in which a system is in thermal equilibrium with its surroundings. A system in thermodynamic equilibrium is in thermal equilibrium, mechanical equilibrium, electrical equilibrium, and chemical equilibrium. A system is in equilibrium when it is in thermal equilibrium with its surroundings.

00:54

In chemistry, chemical equilibrium (also known as dynamic equilibrium) is a state of chemical stability in which the concentrations of the chemical substances do not change in the course of time due to their reaction with each other in a closed system. Chemical equilibrium is an example of dynamic equilibrium, a thermodynamic concept.

05:13

The equilibrium constant f…

00:53

07:56

The following diagram repr…

03:31

03:18

02:06

0:00

01:30

So for this question, we will be using the diagrams in the book a lot. So we want to find the equilibrium concentrations. So what we wanted to first we want to find the K C. Given the concentrations that we have given to us in the book itself, using the diagrams. So in order to do so, we should find first concentration of A to the concentration of B two in the concentration of a product. A. So we have four spheres and we know that each of the spheres is your point is your two moles and we have just one leader. Now that we have the same the diagram, Herbie too there for the product. We have just two. We calculate these out. We find the concentration here to your 0.8 Same for here, and it's only 0.4 here. But given this, we can go ahead and find the Casey, which will aid us later on to do products. Reason how many moles we have over the reactions and calculated out we find this to be 0.25 for the equilibrium constant. So that being said, you wanna look at the diagrams for be and we're gonna fill out an ice table. This is a little bit different than some of the ones we've seen in the past because we're starting out with a known initial concentration for our product, which means starting it with zeros on the reactant side. Which means we're going to subtract X for the reactive. We're gonna add eggs. We're gonna subtract a two x here and just for clarification, says he misspoke. Ah, we're going to add X here and here. Offices were starting with zero. We're gonna see a positive change. We're going to create the reactant because we will be going in the reverse direction. So we see it Equilibrium 0.1 minus two x x x. So since we already found the case, he value here we are able to use that equilibrium constant at least the same for this reaction. And we're going to do the products just how many moles we have over the reactor's. We can simplify this to be 0.1 minus two x squared over X squared, and then we do this out to find X is equivalent to 0.4 and since we have that now we're able to find the equilibrium concentrations for our to react INTs and our project. So both of reactive zehr just x So we know these to be just the Value X, which we just found me. Zero point 04 but a B we need to do 0.1, which was the initial minus two times that 0.0. For that we calculated for X we find the physical to 0.2 Moller.

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