What is the mole fraction of #NO# in a 55.0 L gas cylinder at 30.0°C which comes from a mixture of #N_2# and #NO# if you have 3.238 mol of #N_2# and the gas cylinder has a total pressure of 2.14 atm?
Your strategy here will be to use the ideal gas law equation in order to find the total number of moles present in the mixture, then use the number of moles of nitrogen gas to determine the mole fraction of nitric oxide.
So, the ideal gas law equation looks like this
Since the mixture only contains nitric oxide and nitrogen gas, it follows that the number of moles of nitric acid will be equal to
Now, the mole fraction of nitric oxide will be equal to the number of moles of nitric oxide divided by the total number of moles present in the mixture.
In this case, you have
The answer is rounded to three sig figs.
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To find the mole fraction of NO, you first need to calculate the moles of NO in the mixture. Then, find the total moles of gas in the mixture. Finally, divide the moles of NO by the total moles of gas.

Calculate moles of NO using the ideal gas law: PV = nRT n(NO) = (P_total * V) / (R * T)

Calculate total moles of gas: n_total = n(NO) + n(N2)

Calculate mole fraction of NO: X(NO) = n(NO) / n_total
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When evaluating a onesided 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 onesided 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 onesided 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 onesided 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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