Kinetic theory of gases

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

Expert Solution

The ideal gas equation relating pressure (P), volume (V), and absolute temperature (T) is given as:

PV = nRT

Where, R is the universal gas constant = 8.314 J mol-1K-1

n = Number of moles = 1

T = Standard temperature = 273 K

P = Standard pressure = 1 atm = 1.013 x 105Nm-2

Hence,

V = nRT / P

= 1 x 8.314 x 273 / 1.013 x 105

= 0.0224 m3

= 22.4 litres

Therefore, the molar volume of a gas at STP is 22.4 litres

The molar volume of a gas at STP is 22.4 litres.

Ajay Kumar Gupta answered 3 years ago

Explain the kinetic molecular theory and it's relationship with gases.

From the expressions we derived for the kinetic theory of gases, it can be shown that...

From the expressions we derived for the kinetic theory of gases, it can be shown that the fraction of gas molecules having speeds in excess of a particular speed c is f(c) = 1 + [2*alpha/sqrt(pi)] exp(-alpha2) - erf(alpha) where alpha = c/cm , cm is the most probable speed and erf() is the error function. Consider now 1000 H2 atoms in thermal equilibrium at 0oC. Consider the range of speeds from 0 to 3,000 m/s divided into 100 m/s...

Explain how the kinetic theory of gases can be applied to measure effusion rates?

To be able to predict and calculate properties of real gases. Kinetic molecular theory makes certain...

To be able to predict and calculate properties of real gases. Kinetic molecular theory makes certain assumptions about gases that are, in fact, not true for real gases. Therefore, the measured properties of a gas are often slightly different from the values predicted by the ideal gas law. The van der Waals equation is a more exact way of calculating properties of real gases. The formula includes two constants, a and b, that are unique for each gas. The van...

Apply the Kinetic Theory of gases to explain Boyle's law, Charles' law and Dalton's law ?

Consider the following statements related to the kinetic theory of gases. Use the drop down choices...

Consider the following statements related to the kinetic theory of gases. Use the drop down choices to mark each as either true or false. You must get all five correct at the same time. 1.Gases behave most ideally at low pressures. 2.The average speed of neon atoms at room temperature is greater than the average speed of argon atoms at room temperature. 3.At a given pressure, all gases have the same average molecular speed. 4.Gases behave most ideally at high...

Derive/explain how thermal conductivity can be explained in terms of the kinetic theory of gases.

One of the assumptions of the kinetic molecular theory is that there are no intermolecular forces...

One of the assumptions of the kinetic molecular theory is that there are no intermolecular forces (attractive or repulsive) between gas particles (atoms or molecules). How would the presence of intermolecular forces affect the ideal gas equation (PV = nRT)? Again, in your response, please use terms that a high school senior who hasn’t taken AP chemistry might use.

use the kinetic molecular theory ( matter = particles ) to explain the differences between solid...

use the kinetic molecular theory ( matter = particles ) to explain the differences between solid vs liquid vs gas phase. And describe how particles are behaving during a phase change

Explain Boyle's Law in terms of the kinetic molecular theory. Decreasing the volume means that there...

Explain Boyle's Law in terms of the kinetic molecular theory. Decreasing the volume means that there are less gas molecules in the container, which increases pressure. Decreasing the volume means that at any one instant less molecules will collide with the walls of the container, which increases pressure. Decreasing the volume means that at any one instant more molecules will collide with the walls of the container, which increases pressure. Decreasing the volume means that there are more gas molecules...

Question