If 20.0g of co2 and 4.4g of co2
areplaced in a 5.00 l container at 21oc, what is
thepressure of this mixture of gases?

The given question is incorrect. The correct question is as follows.

If 20.0 g of and 4.4 g of  are placed in a 5.00 L container at , what is  the pressure of this mixture of gases?

Explanation:

As we know that number of moles equal to the mass of substance divided by its molar mass.

Mathematically,   No. of moles =

Hence, we will calculate the moles of oxygen as follows.

       No. of moles =

     Moles of =

                            = 0.625 moles

Now,   moles of

                                      = 0.1 moles

Therefore, total number of moles present are as follows.

Total moles = moles of + moles of

                    = 0.625 + 0.1

                    = 0.725 moles

And, total temperature  will be:

                    T = (21 + 273) K = 294 K

According to ideal gas equation,  

                         PV = nRT

Now, putting the given values into the above formula as follows.

                P =

                   =

                    = atm

                    = 3.498 atm

or,                = 3.50 atm (approx)

Therefore, we can conclude that the pressure of this mixture of gases is 3.50 atm.

the product of the pressure and volume is also constant