Can someone please explain how to do #4 on Test # 1. The questions states
There is an unknown quantity of Xenon in a 25 L container at .50 atm and 27 C. How many grams of Xenon are present?
Test 1 # 4
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Re: Test 1 # 4
You'd have to use the equation PV=nRT since we have pressure, temperature, gas constant R, and the volume. Solve for n which is the amounts of mols of xenon and convert to grams. Make sure your units cancel out and temperature is in kelvin
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Re: Test 1 # 4
You add 273 to the 27 to get temperature in 300 degrees Kelvin, and make sure the correct Rydberg constant is used so the units Kelvin, Liters, and atm cancel.
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Re: Test 1 # 4
You use PV=nRT and then find the number of moles (n). They forgot to give us the molar mass of Xenon on the test but you have to multiply moles by molar mass and it will give you the mass.
Re: Test 1 # 4
You need to use PV=nRT to find the moles of Xe. Remember to convert your given information to the proper units. Then convert the moles to mass using the molar mass from the periodic table.
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Re: Test 1 # 4
use PV = nRT to solve for n which are moles of the gas. Then use the molar mass and the moles you solved for to solve for grams of gas.
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Re: Test 1 # 4
Ideal gas law but make sure you use the value of R that allows you to cancel your units correctly.
Re: Test 1 # 4
Use pV=nrt when plugged in you will then need to calculte the grams from the moles found using the equation
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Re: Test 1 # 4
Use PV=nRT by plugging in pressure, volume, temperature, and R (0.0821 Latm/(molK)). Isolate and solve for n, which will give you the moles of Xenon present, and you can convert to the grams of Xenon using the molar mass of Xenon.
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Re: Test 1 # 4
This one tricked me too! You have to use the ideal gas law, so PV=nRT and just plug everything in. But make sure to convert everything to the right units.
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Re: Test 1 # 4
You use PV=nRT to solve for n. Then use molar mass of Xe to convert n from moles to grams using stoichiometry.
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