Home
Class 11
CHEMISTRY
Determine the total kinetic energy of th...

Determine the total kinetic energy of the molecules of 8.0 g `CH_(4)` at `27^(@)C` in the unit of joule.

Text Solution

Verified by Experts

8.0 g `CH_(4)=(8)/(16)=0.5mol" "CH_(4)[because M_(CH_(4))=16g*mol^(-1)]`
Total enegy of the molecules in 1 mol gas `=(3)/(2)RT`
`theefore`Total kinetic energy of the molecules of 0.5 mol `CH_(4)` gas
`=0.5xx(3)/(2)RT=0.5xx(3)/(2)xx8.314xx(273+27)==1870.65J`.
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER : GASES AND LIQUIDS

    CHHAYA PUBLICATION|Exercise WARM UP EXERCISE|104 Videos

  • STATES OF MATTER : GASES AND LIQUIDS

    CHHAYA PUBLICATION|Exercise QUESTION-ANSWER ZONE FOR BOARD EXAMINATION|51 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    CHHAYA PUBLICATION|Exercise PRACTICE SET|13 Videos

  • STRUCTURE OF ATOM

    CHHAYA PUBLICATION|Exercise PRACTICE SET|15 Videos

Similar Questions

Explore conceptually related problems

Determine the total kinetic energy of the molecule of 1 g CO_(2) at 27^(@)C in the units of erg and calorie. Assume the ideal behaviour of the gas.

Calculate the kinetic energy of per gm molecule of He gas at 27^@C .

Calculate the average kinetic energy in joules of the molecules in 8.0 g of methane at 27^@C .

At 27^(@)C , average translational kinetic energies of the molecules in 8g of CH_(4),8g of O_(2) and 8g of He are overline(in_(1)),overline(in_(2)) and overline(in_(3)) respectively and total kinetic energies of the molecules in these gases are E_(1),E_(2) and E_(3) respectively. which of the following is true-

Calculate the number of molecules is 1cm^3 of an ideal gas at 27^@C . Temperature and 20 mmHg pressure. The average kinetic energy of one molecule of the gas at 27^@C=4 times 10^-14 erg , density of mercury = 13.6 g.cm^-3

At a constant temperature, a vessel of 1 litre capacity contains 10^(23)N_(2) molecules. If the rms velocity of the molecules be 10^(3)m//s , then determine the total kinetic energy of the molecules and the temperature of the gas.

"The total kinetic energy of the molecules in an ideal gas with a volume V at pressure P and temperature T is equal to the total kinetic energy of the molecules present in the same volume of another ideal gas at the same pressure and at temperature 2T"-Justify the statement.

Calculate the temperature at which the average translational kinetic energy of the molecules of a gas will be 1/3 rd of that at 180^@C ?

IF the number of gas molecules in a container in doubled, how will the pressure and the total kinetic energy of the gas molecules of that container change?

At what temperature the average kinetic energy of the molecules of a perfect gas be doubled than that at 20^@C ?