At #627^@"C"# and #"1 atm"#, #"SO"_3# is partially dissociated into #"SO"_2"# and #"O"_2# . If the density of the equilibrium mixture is #"0.925 g/L"#, what is the degree of dissociation?
The idea here is that you need to calculate the average molar mass of the mixture, as this will help you calculate how many moles of sulfur trioxide dissociated to produce sulfur dioxide and oxygen gas.
Your tool of choice will be this equation--I will not derive the equation here!
Here
In your case, this equation will help you calculate the average molar mass of the mixture. Plug in your values to find--do not forget to convert the temperature of the mixture to Kelvin!
Now, it's important to realize that this actually represents the weighted average of the molar masses of each individual gas. In other words, each gas will contribute to the average molar mass in proportion to its mole fraction in the mixture.
The balanced chemical equation that describes this equilibrium looks like this
This is the case because the number of moles of oxygen gas produced will always be half the number of moles of sulfur trioxide that dissociate.
This means that. at equilibrium, the total number of moles of gas present in the reaction vessel is equal to
The mole fraction of sulfur trioxide will be
Similarly, the mole fractions of sulfur dioxide and of oxygen gas will be
This means that the average molar mas of the mixture can be written as
This means that you have
This is equivalent to
which gets you
You can thus say that the degree of dissociation is equal to
I'll leave the answer rounded to two sig figs, but keep in mind that you have one significant figure for the pressure of the mixture.
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The degree of dissociation of SO3 at 627°C and 1 atm, given a density of 0.925 g/L for the equilibrium mixture, cannot be determined without additional information such as the initial concentration of SO3 and the molar masses of SO3, SO2, and O2.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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