Question

Which of the following laws concerning gases is misstated? a. In a mixture of gases, the total pressure of the gases equals the sum of the individual pressures of each gas. b. At fixed temperature and pressure, the volume of a gas is inversely proportional to the number of moles of that gas. c. At fixed pressure, the volume of a gas is directly proportional to its temperature in Kelvin. d. At fixed temperature, the volume of a gas is inversely proportional to its pressure. e. The average translational kinetic energy of the molecules of a gas is directly proportional to the temperature in Kelvin.

Answer 1

Answer:

b. At fixed temperature and pressure, the volume of a gas is inversely proportional to the number of moles of that gas.

Explanation:

Statement b is wrong.

We can prove it by looking at the ideal gas equation:

$pV=nRT$

where

p is the gas pressure

V is the gas volume

n is the number of moles of the gas

R is the gas constant

T is the absolute temperature of the gas

If we have a gas at fixed temperature T and fixed pressure p, then we see that the relationship becomes

$V\propto n$

which means that the volume is directly proportional to the number of moles of the gas: so, the statement is wrong.

Answer 2

b. At fixed temperature and pressure, the volume of a gas is inversely proportional to the number of moles of that gas.

Further Explanation

Boyle's legal statement is the volume of the mass of a given gas inversely proportional to the pressure when the temperature is constant.

Charles's legal statement is the volume (V) of a given gas mass, at constant pressure (Pa), directly proportional to temperature (K).

Gay-Lussac's Law, for a certain mass and constant volume of an ideal gas, the pressure applied to the side of the container is directly proportional to the absolute temperature.

Avogadro's Law states that the volume occupied by an ideal gas is directly proportional to the number of gas molecules present in the container.

The combined gas law or the General Gas Equation is obtained by combining Boyle's Law, Charles's Law, and Gay-Lussac's Law. This equation shows the relationship between pressure, volume, and temperature for a gas with a fixed mass (quantity).

This law has the following important consequences:

• If the temperature and pressure are kept constant, the volume of the gas is directly proportional to the number of gas molecules.
• If the temperature and volume remain constant, the gas change pressure is directly proportional to the number of gas molecules present.
• If the number of gas molecules and temperature remains constant, the pressure is inversely proportional to volume.
• If the temperature changes and the number of gas molecules are kept constant, the pressure or volume (or both) will change in direct proportion to the temperature.

The relationship between temperature, volume and gas pressure

Equation 1 = Volume is inversely proportional to pressure:

V∝1 / P

Equation 2 = Volume is proportional to absolute temperature:

V∝T

Equation 3 = Pressure proportional to absolute temperature:

P∝T

If equation 1, equation 2 and equation 3 are combined together, it will look like this: PV ∝ T → Comparison 4.

This comparison states that pressure (P) and volume (V) are proportional to absolute temperature (T).

Conversely, volume (V) is inversely proportional to pressure (P).

Information :

P = pressure

V = Volume

T = temperature

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Details

Grade:  High School

Subject:  Physic

keywords:  Laws concerning gases