There are always ONE mole of gas in 22,4 L gas of any kind (even gaseous mixtures like air) at stp.
So 68.5 (L) / 22.4 (L/mole) = 3.06 mole gas in 68.5 L (at STP)
67.2 (L) / 22.4 (L/mole) = 3.00 mole of ANY gas at STP
3 moles at STP are present. 1 mole of a gas occupies 22.4 liters at STP. So 67.2/22.4 = 3.
One mole of any gas occupies 22.4 liters of space at standard temperature and pressure. Given 7.31 moles, you simply multiply that by 22.4 and get the answer of 163.74 liters.
The answer is 0,305 moles at 1 at and 25 0C.
2,22 1023 molecules of carbon dioxide is equal to 0,368 moles.
7.30 moles carbon dioxide (6.022 X 10^23/1 mole CO2) = 4.40 X 10^24 molecules of carbon dioxide
2.10 moles carbon dioxide (6.022 X 1023/1 mole CO2) = 1.26 X 1024 molecules of carbon dioxide ==============================
6.23 mol carbon dioxide
3.74 moles CO2 (6.022 X 10^23/1mol CO2) = 2.25 X 10^24 molecules of carbon dioxide.
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
211g of carbon dioxide are equal to 4,794 moles.
2,22 1023 molecules of carbon dioxide is equal to 0,368 moles.
7.30 moles carbon dioxide (6.022 X 10^23/1 mole CO2) = 4.40 X 10^24 molecules of carbon dioxide
2.10 moles carbon dioxide (6.022 X 1023/1 mole CO2) = 1.26 X 1024 molecules of carbon dioxide ==============================
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
= 9403.41
6.23 mol carbon dioxide
3.74 moles CO2 (6.022 X 10^23/1mol CO2) = 2.25 X 10^24 molecules of carbon dioxide.
5
6.32 mol carbon dioxide
B. 6.23 mol carbon dioxide