Question

for a mixture 0.5 moles of helium and 0.3 moles of N2 in a container of 0.8 litre at 27°c. what is the total pressure​

Answer 1

Given:

A mixture 0.5 moles of helium and 0.3 moles of Nitrogen in a container of 0.8 litre at 27°c.

To Find:

What is the total pressure​?

Solution:

We know the value of universal gas constant (R) is given below:

$\mathbf{\bar{R} = 0.0821 \ \dfrac{atm-L}{ mol-K}}$

Total number of moles of gas:

N = 0.5 +0.3 = 0.8 mole

Volume of container is:

$\mathbf{V = 0.8 \ L}$

Temperature of mixture of gas is:

T = 27°C = 273 + 27 = 300 K

From equation of ideal gas:

$\mathbf{PV=N\bar{R}T}$

This can also be written as:

$\mathbf{P=\dfrac{N\bar{R}T}{V}}$

On putting respective value in above equation:

$\mathbf{P=\dfrac{0.8\times 0.0821\times 300}{0.8}}$

On simplify:

P = 24.63 atm

Total pressure of mixture is 24.63 atmospheric pressure.