Question

If the temperature of a volume of ideal gas increases for 100°C to 200°C, what happens to the average kinetic energy of the molecules?

Answer 1

Answer:
`\Delta E=2.0715* 10^(-21) J`

Step-by-step explanation:

Given

Temperature of the gas is increased from 100 to 200

Also we know that average kinetic energy of the molecules is

`E=(3)/(2)\cdot (R)/(N_A)T`

Where

R=Gas constant

`N_A`=Avogadro's number

T=Temperature in kelvin

`(R)/(N_A)=1.381* 10^(-23)`

So kinetic energy increases by

`\Delta E=(3)/(2)* 1.381* 10^(-23)\left ( 200-100\right )`

`\Delta E=2.0715* 10^(-21) J`