If you have 2.2x10^24 molecules of O2 at STP, how many liters of O2 do you have?
Can someone show me how to solve this
1 mol O2 occupies 22.4 L at STP.
How many mols O2 do you have? You know 1 mol O2 at STP contains 6.02E23 molecules so you have
2.2E24/6.02E23 = ?mols.
3.65 moles?
Yes, 3.65 mols O2. You're half way there. The problem asks for the volume. So 1 mol will occupy 22.4 L at STP. How many L will 3.65 mols occupy?
Can you give me a better way to solve it please because I’m a tad bit confused on how to solve for it
If 1 mol O2 occupies 22.4 L at STP then 2 mol O2 will occupy 22.4 x 2 = ? and 3 mols will occupy 22.4 x 3 mol = ? etc.You have 3.45 mol O2. What volume will that occupy.
Look at the dimensional work.
At STP O2 occupies 22.4L so we know that is 22.4 L/mol. So 22.4 L/mol x # mol = ?L
You seem to be letting the "language of chemistry" confuse you. If I told you that 1 apple, cut up into small pieces, had a volume of 1 cup and I wanted to know how many cups 3.45 cut up apples would occupy, you would tell me immediately that it would be 1 cup/apple x 3.45 apples = ? cups. But when we change the units to Liters and mols and use oxygen instead of apples you get confused and don't know what to do. Do you see what I mean? You are letting the words confuse you when common sense tells you what to do. Don't get discouraged. Many students do this at the beginning.
To solve this question, you need to use the ideal gas law equation: PV = nRT. In this equation, P represents pressure, V represents volume, n represents the number of moles, R is the ideal gas constant, and T represents temperature.
Given:
Number of molecules of O2 = 2.2 x 10^24
STP conditions:
Pressure (P) = 1 atm
Temperature (T) = 273.15 K
First, let's find the number of moles of O2. The number of moles (n) can be calculated using Avogadro's number, which states that one mole of any substance contains 6.022 x 10^23 particles (atoms or molecules).
Number of moles of O2 = (Number of molecules of O2) / (Avogadro's number)
= (2.2 x 10^24) / (6.022 x 10^23)
≈ 3.65 moles
Now, we can use the ideal gas law equation to find the volume (V) of O2. Rearranging the equation, we get:
V = (nRT) / P
Substituting the given values:
V = (3.65 moles) x (0.0821 L·atm/(mol·K)) x (273.15 K) / (1 atm)
≈ 77.35 L
Therefore, you have approximately 77.35 liters of O2 at STP.