12.21.2017 | Logan Miers

NTP = normal temperature/pressure = 20°C (68°f) and 1 atm (atmosphere). Avagadro's Law: The **volume** of 1 mole of any gas (stp) = 22.4 liters. This is an.

(STP). ncf = normal cubic foot = 1 c.f. (NTP). 1 gallon = 3.78 liters 1 cubic foot = 7.5 gallons = 28.25 liters. scf = "scuff" = standard cubic foot = 1 c.f.

1 atm = 1 atmosphere = 14.7 psi.

For example, 1 mole of water (H 2 O) has 2 x 1 + 16 = 18 grams mass. The mass of 1 mole of a compound is equal to its atomic weight, in grams. A mole is a certain amount of stuff, defined as 6 x 1023 molecules of the compound (Avagadro's number).

This is an amazing, useful result. Avagadro's Law: The *volume* of 1 mole of any gas (stp) = 22.4 liters.

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4.13.2017 | Jessica MacAdam

The molar **volume**, symbol Vm, is the volume occupied by one mole of a substance at a given temperature and pressure. It is equal to the molar mass (M) divided.

It can be simply the sum of the individual components, and calculated using:. If the sample is a mixture containing N components, the molar *volume* is complex.

It has the SI unit cubic metres per mole (m3/mol), although it is more practical to use the units cubic decimetres per mole (dm3/mol) for gases and cubic centimetres per mole (cm3/mol) for liquids and solids. It is equal to the molar mass ( M ) divided by the mass density (ρ). The molar volume, symbol V m, is the volume occupied by one mole of a substance ( chemical element or chemical compound ) at a given temperature and pressure.

The 2006 CODATA recommended value for the molar volume of silicon is 12.058 ×10−6 m3/mol, with a relative standard uncertainty of 9.1×10−8.

This is related to the molar volume by.

9.18.2017 | Jessica MacAdam

For 1 mole, PV=RT.

The issue is that one mole of a gas at NTP should not be $22.4$ liters based on the ideal gas. This is only true for a gas at STP. The key difference between the two conditions is they are defined by different temperatures (STP is for $273$K while NTP is for $293$K).

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The definition of NTP as given by IUPAC is.

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Why is the above calculation in NTP condition giving wrong results? How else to prove that molar *volume at* NTP is 22.4l?

On putting T=273K and P=1bar(conditions of STP), we get V=22.4 litres.

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See this link from The Engineering ToolBox for more info.

Therefore, molar volume at STP is 22.4litres.

Substituting P=1atm, T=293K, R=0.0821, we get V=24.05 litres as the molar volume.

It is also known that Volume occupied by 1 mole of gas at NTP is 22.4litres.

My attempt at proving the above statement.

They are also different in that the IUPAC now defines STP with respect to $1$ bar while NTP is defined with respect to $1$ atm.

NTP - Normal Temperature and Pressure - is defined as air at 20oC(293.15 K, 68oF) and 1 atm (101.325 kN/m2, 101.325 kPa, 14.7 psia, 0 psig, 29.92 in Hg, 407 in H2O, 760 torr).

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6.15.2017 | Jessica MacAdam

Proving using ideal gas law that molar **volume at** NTP is 22.4 litrs. NTP - Normal Temperature and Pressure - is defined as air at 20oC(293.15 K, 68oF) and 1 atm (101.325 kN/m2, 101.325 kPa, 14.7 psia, 0 psig, 29.92 in Hg, 407 in H2O, 760 torr). It is also known that Volume occupied by 1 mole of gas at NTP is 22.4litres.

The key difference between the two conditions is they are defined by different temperatures (STP is for $273$K while NTP is for $293$K). This is only true for a gas at STP. The issue is that one mole of a gas at NTP should not be $22.4$ liters based on the ideal gas.

On putting T=273K and P=1bar(conditions of STP), we get V=22.4 litres.

They are also different in that the IUPAC now defines STP with respect to $1$ bar while NTP is defined with respect to $1$ atm.

NTP - Normal Temperature and Pressure - is defined as air at 20oC(293.15 K, 68oF) and 1 atm (101.325 kN/m2, 101.325 kPa, 14.7 psia, 0 psig, 29.92 in Hg, 407 in H2O, 760 torr).

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Substituting P=1atm, T=293K, R=0.0821, we get V=24.05 litres as the molar *volume*.

Why is the above calculation in NTP condition giving wrong results? How else to prove that molar volume at NTP is 22.4l?

For 1 mole, PV=RT.

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By posting your answer, you agree to the privacy policy and terms of service. asked 24 days ago viewed 121 times active 23 days ago.

Therefore, molar volume at STP is 22.4litres.

See this link from The Engineering ToolBox for more info.

By subscribing, you agree to the privacy policy and terms of service.

It is also known that Volume occupied by 1 mole of gas at NTP is 22.4litres.

My attempt at proving the above statement.

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The definition of NTP as given by IUPAC is.

3.12.2017 | Logan Miers

"24 L" NIST uses a temperature of 20^@"C" ("293.15 K", 68^@"F") and an absolute pressure of "1 atm" ("14.696 psi", "101.325 kPa").

#T_1 = 273.15 K #

#=> (22.41 L)/(273.15 K) = V_2/(293.15 K)#

#"T = 293.15K"# #P = 1 atm# so.

#V_2 = ? larr "This is the *volume* of 1 mol of a gas at NTP "#

#=> V_2 = (22.41 L)(293.15 K)/(273.15 K) = 24.05 L#

NIST uses a temperature of #20^@"C"# #("293.15 K"#, #68^@"F")# and an absolute pressure of #"1 atm"# #("14.696 psi"#, #"101.325 kPa")#. This standard is also called normal temperature and pressure (abbreviated as NTP).

#"Therefore, 1 mol of any gas will occupy about 24 L at NTP."# Hope this helped.

Normal Temperature and Pressure.

Plugging our information into Charle's Law: #V_1/T_1 = V_2/T_2#

The only difference between STP and NTP is that NTP conditions are at #20^@"C" = "293.15 K"#, rather than at #0^@"C" = "273.15 K"#

Since only the temperature is different, use Charle's Law: #V_1/T_1 = V_2/T_2# We have:

#T_2 = 293.15 K. #.

#V_1 = 22.41 L #

Describe your changes (optional) 200 #"24 L"#