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 \( 9dm^3\) flask at 27°C ?

Asked by Pragya Singh | 1 year ago |  64

1 Answer

Solution :-

It is known that,

p =\( \dfrac{m}{M}\dfrac{RT}{V}\)

For methane (CH4),

\( p_{CH_{ 4 }}\)

\( \dfrac{ 3.2 }{ 16 }​ × \dfrac{8.314 \; \times \;300 }{9 \; \times \; 10^{-3 }}\)

\( [Since \;9dm^3 = 9 \; \times \; 10^{-3}m^3 \;27°C\)

\( = 300 K]\)

= 5.543 × \( 10^{ 4 }\) Pa

For carbon dioxide (CO2),

\( p_{CO_{ 2 }}\)

=\( \dfrac{ 4.4 }{ 44 }× \dfrac{8.314 \; \times \;300 }{9 \; \times \; 10^{-3}}\)

\( 2.771 × 10^{4} Pa\)

Total pressure exerted by the mixture can be calculated as:

\(p= p_{CH_{ 4 }} + p_{CO_{ 2 }}\)

\( (5.543 × 10^{ 4 }+ 2.771 × 10^{4}) Pa\)

\( 8.314 × 10^{ 4 }\) Pa

Answered by Pragya Singh | 1 year ago

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