Question

2 grams of hydrogen & 16 grams of He are mixed at 298K & 1atm pressure. Calculate the molar entropy of mixing (in J) of the mixture formed, assuming ideal behaviour of the gas.​

Answer 1

Answer:

sry i dont know the answer

Answer 2

The molar entropy of the mixture formed will be 5,21J

Explanation:

Given,

Mass of Hydrogen = 2g

Mass of Helium = 16g

Temperature = 298K

Pressure = 1atm

To find,

Molar Entropy

Formula used

Δ$S_{mixing}$ = $-R[x_{A} ln(x_{A}) + x_{B}ln(x_{B} ) ]$

Moles of Hydrogen = $\frac{2}{2} = 1mol$

Moles of Helium = $\frac{16}{4} = 4moles$

Mole fractions,

$x_{A} = \frac{moles of A}{Moles of A + Moles of B}$

$x_{A} = \frac{2}{6}\\\\x_{A} = 0.33$

$x_{B} = \frac{moles of B}{Moles of A + Moles of B}$

$x_{A} = \frac{4}{6}\\\\x_{A} = 0.66$

$-R[x_{A} ln(x_{A}) + x_{B}ln(x_{B} ) ]\\\\\\-R[0.33(ln0.33)+0.66(ln0.66)]\\\\-R[0.33(-1.1)+0.66(-0.4)]\\\\-8.314[-0.363-0.264]\\\\-8.314[-0.627]\\\\5.21$

Therefore, the molar entropy of mixture is 5.21J.