Differences and similarities between liquid and gas
1 answer:
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Answer : The mole fraction and partial pressure of and
gases are, 0.267, 0.179, 0.554 and 1.54, 1.03 and 3.20 atm respectively.
Explanation : Given,
Moles of = 1.79 mole
Moles of = 1.20 mole
Moles of = 3.71 mole
Now we have to calculate the mole fraction of and
gases.
and,
and,
Thus, the mole fraction of and
gases are, 0.267, 0.179 and 0.554 respectively.
Now we have to calculate the partial pressure of and
gases.
According to the Raoult's law,
where,
= partial pressure of gas
= total pressure of gas = 5.78 atm
= mole fraction of gas
and,
and,
Thus, the partial pressure of and
gases are, 1.54, 1.03 and 3.20 atm respectively.
Answer:
A beaker
Step-by-step explanation:
Specifically, I would use a 250 mL graduated beaker.
A beaker is appropriate to measure 100 mL of stock solution, because it's easy to pour into itscwide mouth from a large stock bottle.
You don't need precisely 100 mL solution.
If the beaker is graduated, you can easily measure 100 mL of the stock solution.
Even if it isn't graduated, 100 mL is just under half the volume of the beaker, and that should be good enough for your purposes (you will be using more precise measuring tools during the experiment).
