The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

The volume of a fixed mass of gas is inversely proportional to its pressure at constant temperature . This is known as Boyle’s law. P1 V1=P2 V2 PV =a constant P inversely proportional to 1/V at constant T.

Ideal Gas Law. gives the relation ship between the pressure, volume, temperature, and number of moles for a sample of gas. (The Ideal Gas Law is derived from the Combined Gas Law and Avogadro’s Principle.)

Therefore, we can conclude that the statement product of pressure and volume of an ideal gas is proportional to the absolute temperature, can best be concluded from the ideal gas law.

Which statement can best be concluded from the ideal gas law? The product of pressure and volume of an ideal gas is proportional to the absolute temperature.

Which laws can be combined to form the ideal gas law? C. Charles’s law, Avogadro’s law, and Boyle’s law. Volume is directly proportional to moles (Avogadro’s law) and to temperature (Charles’s law).

V1/T1=V2/T2. V1n1=V2n2.

Which statement would be the most useful for deriving the ideal gas law? Volume is directly proportional to the number of moles.

Ar (Argon) is the gas that occupies the highest volume at STP.

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STP stands for standard temperature and pressure and it is at a temperature of 0 degrees Celsius or at 273 Kelvin and at a pressure of 101.325 kPa or 1 atm. For gases, at this temperature it was established that for every one mol of a gas it is equivalent to 22.414 Liters.

Thus the 3,01*10^23 of oxygen will have the volume of 11.2 liter.

8.25 litres

Explanation: 1 mol of any gas at STP occupies 22.4 litres of volume.

The gram equivalent volume of oxygen at Standard Temperature and Pressure( STP) is​ 5.6 Litre. Explanation: It is already known that 1 mole of the gas( or 32g of O2) is equivalent to 22.4 Litres of the oxygen gas.

The volume of `1kg` of oxygen gas at `NPT` is `0.7m^(3)` .

22.4L

Assuming that the gas is at standard temperature and pressure (STP), one mole of any gas occupies 22.4 L . This means the number of moles of O2 is 222.4=0.089 mol .

Answer: The volume occupied is 33.6 Liters. Explanation: STP conditions are known as standard temperature and pressure.

Explanation: One mole of gas has a volume of 22.4L at STP. Since there are two moles of gas present, the volume is doubled.

The molar volume of a gas is the volume of one mole of a gas at STP. Avogadro’s hypothesis states that equal volumes of any gas at the same temperature and pressure contain the same number of particles. At standard temperature and pressure, 1 mole of any gas occupies 22.4 L.

The ideal gas law accounts for pressure (P), volume (V), moles of gas (n), and temperature (T), with an added proportionality constant, the ideal gas constant (R). The universal gas constant, R, is equal to 8.314 J·K-1 mol-1.

The factor “R” in the ideal gas law equation is known as the “gas constant”. The pressure times the volume of a gas divided by the number of moles and temperature of the gas is always equal to a constant number. The numerical value of the constant depends on which units the pressure volume and temperature are in.

If we measure pressure in kilopascals (kPa), volume in litres (L), temperature in Kelvin (K) and the amount of gas in moles (mol), then we find that R = 8.314 and it has the units kPa L K-1 mol-1.

the law that the product of the pressure and the volume of one gram molecule of an ideal gas is equal to the product of the absolute temperature of the gas and the universal gas constant.

In physics, the gas constant is defined as the product of pressure and volume. Denoted by R and expressed as energy per temperature increase per mole. The value of R in atm is constant….Value Of R.