A cubic decimeter is a liter, so we're talking 50L of oxygen gas at STP. 1mol of any gas at STP occupies 22.4L of space, so 50/22.4 = about 2.2mol of oxygen.

At STP, one mole of any gas occupies 22.4 liters. This is called molar volume. 113.97 liters Ã· (22.4 L/mol) = 5.09 moles Then convert moles to molecules (1 mole = 6.02 Ã— 1023 molecules) 5.09 moles Ã— (6.02 Ã— 1023 molecules/mol) = 3.06 Ã— 1024 molecules

O.8 moles of 122.4 L of neon at STP.

at stp 1 mole of a gas contains 22.4 litres. 9.1/22.4= .40625 moles o2. 1 mole of a gas contains 6.022E23 molecules so .40625 moles x 6.022E23 = 2.4464325E23 molecules, but you have to multiply by two due to it being diatomic, so answer x 2 = 4.892875E23 molecules

8,4 liters of nitrous oxide at STP contain 2,65 moles.

16,8 L of Xe gas at STP is equivalent to 0,754 moles.

at STP 1 mole occupies 22.4 litres. 64.28 / 22.4 is 2.8696428 moles. Multiply this by avagadro's constant (6.022*10^23) gives 1.7281x10^24 molecules

22.4 liters will have 1 mole of Helium at STP. So, 6 liters will have 0.23 moles

At STP/NTP, 10dm3 of oxygen contains 0.45 moles

1,75/21,4 = 0,0818 moles

The answer is 0,2675 moles.

The answer is 2,68 moles.

Assuming ideal behaviour, 1 mole of any gas occupies 22.4L at STP. So, moles of 10L = 10/22.4 moles = 0.4464 moles

The volume of 5.0 moles of 02 at STP is 100 litres.

Gas has the common formula of C8H18. This gives it a molar mass of 114.229 grams per mole, so there are 276 moles. This is equal to 1.662 E26 molecules.

The answer is 0,305 moles at 1 at and 25 0C.

3 moles at STP are present. 1 mole of a gas occupies 22.4 liters at STP. So 67.2/22.4 = 3.

The amount of oxygen is 0,067 moles.

At STP 1mol O2 = 22.4L 1mol O2 = 6.022 x 1023 molecules O2 22.4L O2 = 6.022 x 1023 molecules O2 Convert liters O2 to moles O2 3.36L O2 X (6.022 x 1023 molecules O2/22.4L O2) = 9.03 x 1022 molecules O2

1 mole occupies 22.4 liters at STP so 44.8/22.4 = 2 moles so 2 x 6.022 x 1023 so 12.044 x 1023 or 1.2044 x 1024

1 mole of gas occupies 22.4 liters at STP. 564/22.4 = 25.18 moles (2 decimal places)

1 mole = 22.414 liters So, 5 moles = 112.07 liters

At STP, 1 mole of any ideal gas occupies 22.4 liters. Therefore, 5 liters of NO2 at STP will represent 0.22 moles (5/22.4), and this is the case for any other ideal gas. So, the answer is that 5 liter of ANY ideal gas will have the same number of molecules as 5 liters of NO2.

At STP, one moles will occupy 22.4 liters.

0.43 moles, since 1 mole of gas occupies 22.4 L at STP.

I never remember STP conversion factors, so PV = nRT will have to do. (1atm)(11.2L) =(n)(0.08206 Latm/molK)(298.15K) = 0.458 moles H2 (6.022 X 10^23/1mol H2) = 2.76 X 10^23 molecules of Hydrogen ( in diatomic form )

67.2 (L) / 22.4 (L/mole) = 3.00 mole of ANY gas at STP

The answer is 2,5 moles.

The number of argon moles is 0,25.

1 MOLE of gas occupies 22.4 Liters at STP so a 4 liter flask conatins 4/22.4 = 0.1786 moles

The answer is 8,5379.10e23 molecules.

The answer is 4,1 CO2 moles.

At standard temperature and pressure (STP), 1 mole of any gas occupies about 22.4 liters of space. If you have 3.75L of a gas, then 3.75/22.4=0.17 moles.

1 mole of an ideal gas occupies 22.4 liters at STP - so 2 moles occupies 44.8 liters.

Ideal gas equation. PV = nRT ===============

density= mass/ volume. number of moles= volume x RTP or STP

That will depend on the temperature and pressure. At STP, you will have 5x22.4 = 112 liters

Assuming that this ammonia gas is at STP, you can use Avogadro's number to gind the number of moles of gas: (387 x 1021 molecules) x (1 mol / 6.02x1023particles) x (17.03 g / 1 mol) =110 g NH3

1 mole of any gas at STP is 22.4L, so 22.4L of nitrogen gas is 1 mole of nitrogen gas.

The volume is 19,48 L.

1.12 X10 to the 23rd power molecules SO2

1 mole occupies 22.4 liters. So 2/22.4 = 0.0893 moles

You find the answer by mulitplying the 8 moles by 22.4, L/mol, which is the volume of any one mole of gas at STP. So the answer is 179.2 L

Chlorine, as a gas it's Cl2, in period 3 exists as diatomic molecules at STP.

Molecules of I2 have stronger intermolecular forces than molecules of Br2

In STP a mole has a volume of 22.4dm3.so 1.5 mole has a volume of 33.6dm3

22.4L=1 mole of gas at STP

For gases, at STP, 1 mole = 22.4L.

5.6 dm3 is divided by 22.4 dm3 to give number of moles: =5.6dm3/22.4moles per dm3 =0.25 moles So 0.25 moles of C3H4 react.

PV = nRT ⟹ n = PV/RT = 1 * 18.65 / (0.082 * 273.15) = 0.8321 moles.

We use, PV =nRT. (1 atmosphere)( 44.8 L) = n(0.08206 L*atm/mol*K)*(298.15 K) 44.8/24.4662 = 1.831 moles of said gas ---------------------------------------now, 1.831 moles of said gas (6.022 X 1023/1 mole said gas) = 1.10 X 1024 molecules of said gas ----------------------------------------------