All gasses deviate from gas laws at

Question

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Answer 1

At high pressure and low temperature, the molecular interaction terms become significant.
So, we cannot neglect these terms.
Also, the total size of molecules becomes significant at low temperatures.
So, at low temperature and high pressure, there is a significant deviation from ideal gas equation.

Answer 2

At high pressure and low temperature, the molecular interaction terms become significant.
So, we cannot neglect these terms.
Also, the total size of molecules becomes significant at low temperatures.
So, at low temperature and high pressure, there is a significant deviation from ideal gas equation.

All gasses deviate from gas laws at

high pressure and low temperature.

low pressure and high temperature.

high pressure and high temperature.

low pressure and low temperature.

At high pressure and low temperature, the molecular interaction terms become significant.
So, we cannot neglect these terms.
Also, the total size of molecules becomes significant at low temperatures.
So, at low temperature and high pressure, there is a significant deviation from ideal gas equation.

A real gas behaves as an ideal gas :

A real gas can be approximated to an ideal gas at

A sample of $O_{2}$ gas and a sample of hydrogen gas both have the same no. of moles, the same volume and same pressure. Assuming them to be perfect gases, the ratio of temperature of oxygen gas to the temperature of hydrogen gas is :

The molar gas constant is the same for all gases because at the same temperature and pressure, equal volumes of gases have the same :

An ideal gas is that which

Revise with Concepts

Ideal Gas Equation and Absolute Temperature

All gasses deviate from gas laws at

high pressure and low temperature.

low pressure and high temperature.

high pressure and high temperature.

low pressure and low temperature.

At high pressure and low temperature, the molecular interaction terms become significant.So, we cannot neglect these terms.Also, the total size of molecules becomes significant at low temperatures.So, at low temperature and high pressure, there is a significant deviation from ideal gas equation.

A real gas behaves as an ideal gas :

A real gas can be approximated to an ideal gas at

A sample of O2​ gas and a sample of hydrogen gas both have the same no. of moles, the same volume and same pressure. Assuming them to be perfect gases, the ratio of temperature of oxygen gas to the temperature of hydrogen gas is :

The molar gas constant is the same for all gases because at the same temperature and pressure, equal volumes of gases have the same :

An ideal gas is that which

Revise with Concepts

Ideal Gas Equation and Absolute Temperature

At high pressure and low temperature, the molecular interaction terms become significant.
So, we cannot neglect these terms.
Also, the total size of molecules becomes significant at low temperatures.
So, at low temperature and high pressure, there is a significant deviation from ideal gas equation.

A sample of $O_{2}$ gas and a sample of hydrogen gas both have the same no. of moles, the same volume and same pressure. Assuming them to be perfect gases, the ratio of temperature of oxygen gas to the temperature of hydrogen gas is :