#### Question

Calculate the volume occupied by 8.8 g of CO_{2} at 31.1°C and 1 bar pressure.

R = 0.083 bar L K^{–1} mol^{–1}.

#### Solution 1

It is known that,

`pV = m/M RT`

`=> V = (mRT)/(Mp)`

Here

*m* = 8.8 g

R = 0.083 bar LK^{–1} mol^{–1}

*T* = 31.1°C = 304.1 K

*M* = 44 g

*p* = 1 bar

Thus volume (V) = `(8.8 xx 0.083 xx 304.1)/(44xx1)`

= 5.04806 L

= 5.05 L

Hence, the volume occupied is 5.05 L.

#### Solution 2

No of Mole of `CO_2 (c)` = `("Mass of " CO_2)/"Molar Mass"`

`= (8.8 g)/(44g mol^(-1)) = 0.2 mol`

Pressure of `CO_2 (P) = 1 "bar"`

`R = 0.083 "bar " LK^(-1) mol^(-1)`

Temperature (T) = 273 + 31.1

= 304.1 K

Since from gas equation PV = nRT

V = nRT/P = `(0.2 xx 0.083 xx 304.1)/ (1 "bar")`

= 5.048 L

Is there an error in this question or solution?

Solution Calculate the Volume Occupied by 8.8 G of Co2 at 31.1°C and 1 Bar Pressure. R = 0.083 Bar L K–1 Mol–1. Concept: Behaviour of Real Gases:- Deviation from Ideal Gas Behaviour.