Question

Boltzmann’s constant is 1.38066 × 10−23 J/K, and the universal gas constant is 8.31451 J/K · mol.

Answer 1

Answer:

$4.95\cdot 10^{-21} J$

Explanation:

First of all, let's convert everything into SI units:

n = 2.4 mol (number of gas moles)

$p=11 atm = 1.11\cdot 10^6 Pa$ (gas pressure)

$V=4.3 L=4.3\cdot 10^{-3} m^3$ (gas volume)

R = 8.31451 J/K · mol (gas constant)

The ideal gas equation states that

$pV=nRT$

Solving for T, we find the gas temperature

$T=\frac{pV}{nR}=\frac{(1.11\cdot 10^6)(4.3\cdot 10^{-3})}{(2.4)(8.31451)}=239.2 K$

And now we can find the average kinetic energy of the gas:

$E_K = \frac{3}{2}kT$

where

k = 1.38066 × 10−23 J/K is the Boltzmann's constant

Substituting,

$E_K = \frac{3}{2}(1.38066\cdot 10^{-23} J/K)(239.2 K)=4.95\cdot 10^{-21} J$