Question

What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm³ flask at 27 °C ?

Answer 1

It is known that,

`"p" = "m"/"M" "RT"/"V"`

For methane (CH­₄),

`"p"_("CH"_4) =  3.2/16 xx (8.314 xx 300)/(9xx10^(-3)) [("Since"  9" dm"^3 = 9xx 10^(-3) "m"^3),(27^@ "C" = 300 " K")]`

` = 5.543 xx 10^4 "Pa"`

For carbon dioxide (CO₂),

`"p"_("CO"_2) = 4.4/44 xx (8.314 xx 300)/(9xx10^(-3))` 

Total pressure exerted by the mixture can be obtained as:

`"p" = "p"_("CH"_4) + "p"_("CO"_2)`

`= (5.543 xx 10^4 + 2.771 xx 10^4)"Pa"`

`= 8.314 xx 10^4 "Pa"`

Hence, the total pressure exerted by the mixture is 8.314 × 10⁴ Pa.