## Properties of Gases Molecule

**Physical properties of gases** are characterized by a lack of definite volume and density and in the gaseous state, the matter has the property of filling completely any available space to uniform density. The low density, high compressibility and thermal energy much greater than the force of attraction are also important properties of the gas molecules. Among crystalline solid, liquid, and gaseous state of aggregation, the gases are allowed for the comparative study between mass, pressure, volume, and temperature. These properties of ideal gases evident to the formation of Boyle’s, Charles, Avogadro law, Gay Lussac, and Graham’s law which provide the relation between mass, pressure, volume, temperature, density, and specific heat of gas molecules for learning chemistry or physics.

The formula in which concerns these four variables is known as ideal gas law. After knowing these experimental ideal gas laws, a theoretical model-based structure of gases developed in kinetic theory which provides the relation between pressure, volume, and velocity of gas molecules.

### Boyle’s Law for Gases Properties

Boyle’s law states as, at a constant temperature, the volume of a definite mass of a gas is inversely proportional to its pressure. Therefore, the volume of a given quantity of gases, at constant temperature equilibrium with the pressure of gases. At constant temperature and 1 atm pressure, a cylinder contains 10 ml of methane or hydrogen gas. If the pressure increases to 2 atm then according to this law volume decreases to 5 ml.

### Boyle’s Law of Gases Formula

According to the definition of Boyle’s law at a constant temperature (T), V ∝ 1/P. Therefore, PV = K = constant for a gas. The value of the gas constant depends on the base properties and mass of the gas molecules. For a given mass of gas, the volume V_{1} at pressure P_{1} and V_{2} at pressure P_{2}. Therefore, according to Boyle’s Law, P_{1}V_{1} = P_{2}V_{2}.

### Pressure Volume Graph of Gas

The relation between pressure and volume of gas can be represented by an arm of a rectangular hyperbola graph given below.

The value of gas constant changes with temperature. Therefore, there will be a separate two-dimension curve for each fixed temperature. When these curves plotted at different fixed temperatures called isotherms. At constant temperature, a given mass of gas is the product of pressure and volume. If the product of pressure and volume of gas represents on y-axis and pressure represents the x-axis a straight-line graph is obtained parallel to the x-axis.

### Pressure and Density of Gas Molecule

Let at a constant temperature, M mass of gas has pressure P_{1} at volume V_{2} and pressure P_{2} at volume V_{2}. According to Boyle’s law of gases formula, P_{1}V_{1} = P_{2}V_{2}; or, P_{1}/P_{2} = V_{2}/V_{1}. Let the density of the gas D_{1} at pressure P_{1} and D_{2} at pressure P_{2}. Therefore, D_{1} = M/V_{1} and D_{2} = M/V_{2}; or, V_{1} = M/D_{1} and V_{2} = M/D_{2}. Putting the value on gas formula, P_{1}/P_{2} = V_{2}/V_{1} = D_{1}/D_{2}; or, P ∝ D. Therefore, at a constant temperature, the density of a definite mass of gases proportional to its pressure.

### Pressure and Volume of Gas

At constant pressure a given mass of gas, volume increases with the increasing temperature. Hence the volume of a given mass of gases at constant pressure is directly proportional to its kelvin temperature.

### Charles law of Gases Properties

Charles law evident the physical properties of the volume of a fixed mass of gases at the various temperature at constant pressure. At constant pressure, each degree rise in temperature of a definite mass of gas expands 1/273.5 of its volume at 0⁰C. Let V_{0} = volume at 0⁰C, then 1⁰C rise of temperature the volume of the gas rise V_{0}/273.5 ml. It is convenient to use the absolute temperature scale on which temperature is measured in Kelvin. Hence the reading on this scale was obtained by adding 273 to the Celsius value. Therefore, TK = 273 + t°C. Therefore, the Charles law represented as V_{t} = (V_{0} × T)/273 = (V_{0}/273) × T.

Since V_{0} = initial volume = constant at a given pressure. Hence the above relation is expressed as, V_{t} = K_{2} T, where K_{2} = constant. Therefore, according to this equilibrium gas formula, Charles law states as, at constant pressure, the volume of a given mass of gases is directly proportional to its kelvin temperature.

### Volume Temperature Graph for Gases

A typical property of the volume of gases with a change in its kelvin temperature a straight-line isobar graph obtained. Thus the general term isobar, which means at constant pressure assigned to these plots.

### Absolute Zero Temperature of Gas Molecules

Since volume is directly proportional to its kelvin temperature. Thus the volume is theoretically zero at zero kelvin or – 273°C. This is hypothetical because the molecule of our environment has physical properties to form liquid and then solid before this low temperature of gas reached. In reality, no substance exists as gases at a temperature near kelvin zero. For the liquefaction of real gases, we must maintain critical temperature.

### Temperature and Density of Gases

Let at constant pressure, for M mass has volume V_{1} at temp T_{1} and V_{2} at temp T_{2}. According to Charles law, V_{1}/V_{2} = T_{1}/T_{2}. Again let the density D_{1} and D_{2} at V_{2} and V_{1 }respectively

Therefore, T_{1}/T_{2} = V_{1}/V_{2} = D_{2}/D_{1}; or, D ∝ 1/T. According to the above formula, at constant pressure, the density of a given mass of gases inversely proportional to its temperature.

### Combined Gases Laws Properties

Charles law, V ∝ 1/P when T constant and Boyle’s law, V ∝ T when P constant in chemistry or physics. Therefore, when all the variables are taken into account the variation rule states as, PV = KT. All gases have properties to obey the gas laws formula under all conditions of temperature and pressure but for real gases or Van der Waals gases, Boyles law, Charles law, and combined laws are approximately applicable only at low pressure and moderately high temperatures.