At STP 1 mole of every gas has the volume of 22.4 dm3. (1 dm3 = 1 L)
According to previous law,
1 mol - 22.4 dm3
x - 5.68 dm3
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x = 0.2536 mol
1 mol of NO weights 30 g (Ar for N is 14, and Ar for O is 16. Mr(NO) = Ar(N) + Ar(O)), so
1 mol - 30 g
0.2536 mol - x
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x = 7.6080 g
So the mass of 5.68 L of NO at STP is 7.6080 grams.
The mass of 43,7 L of helium at STP is 7.8 g.
6.70 g
The mass is 3,358 kg.
13 L of FeO2 can be produced from 50.0 L of O2 at STP.
The molar volume at STP(22.4 L/mol) can be used to calculate the molar mass of the gas.
The mass of 43,7 L of helium at STP is 7.8 g.
At Standard Temperature and Pressure (STP), which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere pressure, the molar volume of an ideal gas is approximately 22.4 liters/mol. The molar mass of nitrogen gas (Nā) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: ļæ½ = Molar mass Molar volume at STP D= Molar volume at STP Molar mass ā ļæ½ = 28.02 ā g/mol 22.4 ā L/mol D= 22.4L/mol 28.02g/mol ā ļæ½ ā 1.25 ā g/L Dā1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
1 standard volume of 1 mole of any gas @ STP is 22.4 LSo the # of moles in a 1 L sample will be:1 L*(1 mol/22.4 L) = 0.04464 molSince you already know the mass of the gas @ STP, the molar mass will be mass/#moles1.92 g/ 0.04464 mol = 43.01 g/mol
6.70 g
The weight of 75.0 L of helium depends on the temperature and pressure at which it is measured. At standard temperature and pressure (STP), which is 0Ā°C and 1 atmosphere, the molar mass of helium is 4.0 grams per mole. Using the ideal gas law, we can calculate the weight by multiplying the molar mass of helium by the number of moles, which is the volume divided by 22.4 L (molar volume at STP). However, if the temperature and pressure are not at STP, additional information is needed to determine the weight.
The mass is 3,358 kg.
Neon, as its mass is 20.18 and Nitrogen's is 14.01
Molar mass of propane = 44 g/mole ... 100 / 44 = 2.727 moles one mole occupies 22.4 L at STP .... 22.4 x 2.727 = 50.91 L
13 L of FeO2 can be produced from 50.0 L of O2 at STP.
mass of CaCO3 = 246 grams
3.61g/L D=m/v
One liter of ozone gas at 1 atmosphere and 0°C has the mass of is 2.141 gm. At 20°C (STP) that would be 1.995 gm. 3.36 L would be 6.70 gm (to three sig figs).