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At $1000 \mathrm{K},$ a sample of pure $\mathrm{NO}_{2}$ gas decomposes:$$2 \mathrm{NO}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)$$The equilibrium constant $K_{P}$ is $158 .$ Analysis shows that the partial pressure of $\mathrm{O}_{2}$ is 0.25 atm at equilibrium. Calculate the pressure of $\mathrm{NO}$ and $\mathrm{NO}_{2}$ in the mixture.

$$\begin{array}{l}P_{\mathrm{NO}}=0.50 \mathrm{atm} \\P_{\mathrm{NO}_{2}}=0.020 \mathrm{atm}\end{array}$$

Chemistry 102

Chapter 14

Chemical Equilibrium

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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.

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At $1000 \mathrm{~K}$, a s…

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A flask containing pure $\…

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The equilibrium constant, …

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The reaction$$2 \mathr…

00:41

The reaction $$2 \mathrm{N…

The equilibrium $2 \mathrm…

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06:48

At $1100 \mathrm{K}, K_{\m…

So we want to find the partial pressure of all of our products and all over react. It's that are in the gaseous form. And thankfully, all over products directives are in the gases form for this balance chemical equation. So in order to find the partial pressures of each substance we see here, we're gonna use the fallen equal a room constant equation. So in order to find this KP value, we're gonna take the partial pressure of our first product raised. How many moles We have partial pressure of our second product. And since we have a one here, this would be raised to the power of one understood that anything raised to the power of one is just itself. And then this will be all over partial pressure, our singular reactant. Just how many rules we have, which is to, as we see here, we were given in the problem that the KP for this balance equation is 158. You were also given partial pressure. Auction, which is one of our products here, is equivalent to zero point 25 That being said, they're also able to find the pressure of our second product. Since this is an equilibrium and based on the story geometry of this balance equation, we know that we can do two times the value that we saw for the oxygen in the pressure of our last product will be 0.5. So now that we have these two values for our products, you go ahead and put them into our KP equation to find the partial pressure over reacted. So this is 0.5 racing power to having moles. You have multiplied with partial pressure of oxygen, our second product all over the partial pressure of our react, which we do not know yet. That's what we're looking for. Now we know this equals 158. So we rearrange this equation, you see that 0.5 squared times 0.25 all over 100 58. Suppose flint to the pressure partial pressure of our reactant raised to how many moles we have. And if you calculate this out, we find that the partial pressure overreacted. Was it willful? It too 0.0 20 a team in the units for our pressure of both of her products are also in a t m.

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