Question

A 10 liter flask at 298 K contains a gaseous mixture of CO and CO2 at a total pressure of 2.0 atm. Of 0.20 mole of CO is present, find the partial pressure of CO and that of CO2.

Answer 1

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Answer 2

Explanation:

The given data is as follows.

   V = 10 L,     T = 298 K,   and   P = 2 atm

So, according to the ideal gas equation PV = nRT where, R = 0.0821 atm L/mol K.

Hence, put the given values into the above formula as follows.

                         PV = nRT

     $2 atm \times 10 L$ = $n \times 0.082 atm L/mol K \times 298 K$

                    n = 0.82 mol

As moles of CO are given as 0.20 mol and total number of moles calculated are 0.82 mol.

Therefore, number of moles of $CO_{2}$ are (0.82 - 0.20) mol = 0.62 mol.

Thus, partial pressure of CO will be calculated as follows.

                         p = $x_{1}p^{o}$

                             = $\frac{\text{no. of moles}}{\text{total number of moles}} \times p^{o}$

                $\frac{0.20 mol}{0.82 mol} \times 2 atm$

                       = 0.4878 atm

Also, partial pressure of $CO_{2}$ is calculated as follows.

                 $\frac{0.62 mol}{0.82 mol} \times 2 atm$  

                       = 1.51 atm