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 $dm^{3}$ flask at 27°C ?

Answer 1

Molar mass of Methane ${ CH }_{ 4 }$ = 16g  

Number of moles of Methane ${ CH }_{ 4 }$ = $\frac { mass }{ Molar\quad mass }$  

$= \frac { 3.2g }{ 16g } =0.2 \quad moles$

Molar mass of Carbondioxide ${ CO }_{ 2 }$ = 44g  

Number of moles of Methane ${ CO }_{ 2 }$ = $\frac { mass }{ Molar\quad mass }$

$= \frac { 4.4g }{ 44g } =0.1 \quad moles$

Therefore, total number of moles = 0.2 + 0.1 = 0.3 moles  

Now, PV = nRT  

${ P= }\frac { nRT }{ V } =\frac { 0.3\times 0.082\times 300 }{ 9 } =\frac { 0.1\times 0.082\times 100 }{ 1 } =0.82\quad atm$

The pressure exerted is 0.82 atm  

Answer 2

HEY MATE...

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THE PRESSURE EXERTED IS 0.82atm

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