Question

Which of the following is true about a 0.200 mol sample of nitrogen gas and a 0.200 mol sample of argon gas that are at 1.20 atm and an initial temperature 55.0 °C when the temperature changes to 400 K? Assume constant volume for the container under both of these temperature conditions.

Group of answer choices

None of these choices is correct

The density of both gases will increase.

There will be more collisions between the gas molecules and the pressure in the container will decrease.

The average kinetic energy of both gases decreases.

The root mean square speed of the gas molecules remains the same.

Answer 1

The Correct Option will be :

• None of these choices is Correct.

because, i) The Density will remain constant, since the gases are kept under constant Volume.

ii) The No. Of Collisions will increase, with increase in Temperature and thus the Pressure will also increase.

iii) The Average Kinetic Energy is directly proportional to the Temperature and will increase with rising Temperature.

iv) Root Mean Square speed is proportional to the Square-Root of the Temperature and thus it will increase with increase in Temperature.