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A mixture of 0.47 mole of $\mathrm{H}_{2}$ and 3.59 moles of $\mathrm{HCl}$ is heated to $2800^{\circ} \mathrm{C}$. Calculate the equilibrium partial pressures of $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ if the total pressure is 2.00 atm. For the reaction$$\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)$$$K_{P}$ is 193 at $2800^{\circ} \mathrm{C}$

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$$\begin{array}{l}P_{\mathrm{H}_{2}}=0.29 \mathrm{atm} \\P_{\mathrm{Cl}_{2}}=0.051 \mathrm{atm} \\P_{\mathrm{HCl}}=1.67 \mathrm{atm}\end{array}$$

Chemistry 102

Chapter 14

Chemical Equilibrium

Carleton College

University of Central Florida

Brown University

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.

02:12

A mixture of 0.47 mol…

01:54

The equilibrium constant $…

So for the following balanced chemical equation, we want to find what the partial pressure is for each of the species in this reaction. So what we want to do first is we want to find the moles at equilibrium. So you will do ice table were given so far, starting moles. We know that for hydrogen it is 0.47 have no initial moles of Corinne. And for a product 3.59 we're gonna do a minus two extra product, plus a singular X processing your ex. That means that equal when we have it's your point or seven plus x x 3.59 minus two X. So now we can plug these into a KP equation. We're gonna do our products based on our story laundry we're gonna raises to a power of two. They were going to dio our first reactant hydrogen times are a second chlorine, and we know that this equals 1 93 because we were given that in the problem itself. So if we were to solve this, we would find that X is a Poland to zero point 10 So since we know this, we can now find equilibrium moles of H two c L two in HCL. So to find our hydrogen, we know we had 0.47 initial plus the X which we hunted the 0.10 trees. We have 0.57 moles for Corinne. We have 0.10 MOL because we just had the X then for our product, we have 3.59 minus to times 0.10 which is equivalent to 3.3 nine. So now that we have these mole values were wanting to find partial pressure, and it's important to keep in mind what are partial pressure equation is defying partial pressure. You do the mole fraction times the pressure total. So let's start finding some mole fractions. So I'll start right here. We need to find the mole fraction of H two, c l two and HCL our product. So to find the mole fraction you take how many moles we have a little bit zero point 57 divided by the total number of moles and you find the total number moles by adding these up, and that is equivalent to 4.6 and then we have 0.10 over 4.6 I am for a product. We have 3.39 over 4.6 So for hydrogen, this is equivalent to 0.14 her chlorine. This is what what to 0.25 Which makes sense, considering how small this value is on top on the numerator. Now then, for the wrong, we have 0.83 And since these are our mole fractions, you can now plug them into this equation that we talked about earlier to find the partial pressure of hydrogen, the partial pressure of chlorine gas and the partial pressure of HCL hydro court guests. So we know that we have 0.14 times our total pressure of to 0.25 has your total pressure of to in 0.83 times are total pressure of to and this is equivalent to 1.7 a. T. M. 0.5 a. T. M. And 0.2 eight a. T. M. And the years are your pressure partial pressure values for this whole balanced equation that we started with

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