One kilomole Ar and one kilomole O2 are heated at a constant pressure of 100 kPa to 3200 K where

One kilomole Ar and one kilomole O2 are heated at a constant...

Key Concepts

Chemical Equilibrium

Chemical equilibrium describes the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of the reactants and products over time. This concept is key in understanding how reactions reach a steady state under a given set of conditions, such as temperature and pressure.

Equilibrium Constant

The equilibrium constant is a numerical value that relates the concentrations or partial pressures of the products and reactants at equilibrium for a reversible reaction. It is crucial for predicting the extent of a reaction and is typically a function of temperature, indicating how changes in conditions can shift the balance between different species.

Mole Fraction

Mole fraction is the ratio of the number of moles of a particular component to the total number of moles in the mixture. It is an important concept in chemical thermodynamics and gas mixtures because it provides a way to express the composition of a system independent of the total amount of material present.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction, determined by their balanced chemical equation. It is essential for understanding how the amounts of different species change as the reaction proceeds, including how the dissociation or formation of molecules affects the overall system composition.

Inert Gas Behavior in Reactions

An inert gas in a chemical reaction is one that does not participate in the reaction itself but can affect the overall mixture's properties such as total pressure and mole fractions. Recognizing the role of an inert component is important when applying equilibrium concepts, as it alters the dilution and partial pressure relationships of the reactive species.

Transcript

00:01 Here we have one, we're told we have one kilomole of oxygen, one kilomole of argon.

00:06 So we actually have an absolute basis here, but it doesn't matter because we're looking for ratios anyway.

00:13 And it's heated up to, i didn't write the temperature here, it's heated up to t equals 3 ,200 kelvin.

00:26 And we're at atmospheric pressure.

00:31 All right.

00:31 So we can look up k for the dissociation of oxygen, and the natural log is minus 3 .04 -07.

00:43 And so the number of total moles here in the, in the equilibrium, we have, let's see here, we have, well, we have, we can look, we can basically cancel out the argons.

01:00 The argon, we're not worried about the dissociation of that.

01:03 What we can't, i mean, we're not, we're not worried about the ionization of that.

01:08 We can't really associate it.

01:10 But at 3 ,300 calvin, i'm pretty sure that there's very, very little ionization of the argon.

01:18 Now, we could, so we're just looking at the oxygen dissociation.

01:24 So we have one over here, and then we have one minus x over here and 2x over here.

01:31 So we have a total number of moles of 2 plus x because over here.

01:42 So we have, yeah, let's see, yeah.

01:46 So we have a total number of moles of the argon.

01:50 So we wind up with the two here because we have this extra argon over.

01:54 If we got rid of the argon, this would be a 1.

01:57 So we changed that by having the argon in the picture...