Question

Pressure of a mixture of $4g$ of $O_2$ and $2g$ of $H_2$ confined in a bulb of $1$ litre at $0^{o}C$ is:

• A. $25.215$ atm
• B. $31.205$ atm
• C. $45.215$ atm
• D. $15.210$ atm

Answer 1

Answer: (A)

$25.215$ atm

Given:

$V=1L$

$T=273K$

Let us find the Partial pressure of O₂.

No. of moles =$4/32=0.125moles$

$P_1$ $=\frac{nRT}{v}=$ $0.125\times 0.082\times \frac{273}{1}=2.80atm$

Now let us find the partial pressure of H₂.

$P_2$= $\frac{nRT}{v}=1\times 0.082\times \frac{273}{1}=22.386atm$

Total pressure of the mixture = $2.80+22.38=25.18atm.$

Therefore $25.18$$\approx$ $25.21$