Calculate the volume occupied by 8.8 g of CO2 at 31.1°C and 1 bar pressure. R = 0.083 bar dm3 K–1 mol–1

Asked by Pragya Singh | 1 year ago |  92

##### Solution :-

pVM = mRT

V = $$\dfrac{mRT}{Mp}$$

Given:

m = 8.8 g

R =$$0.083 \;bar\; dm^{ 3 }at \;K^{-1} mol^{-1}.$$

T = 31.1°C = 304.1K

M = 44 g

p = 1 bar

Thus, Volume (V),

$$\dfrac{8.8 \; \times \; 0.083 \; \times \; 304.1}{ 44 \; \times \; 1}​$$

= 5.04806 L

= 5.05 L

Therefore, the volume occupied is 5.05 L.

Answered by Abhisek | 1 year ago

### Related Questions

#### Explain the physical significance of Van der Waals parameters.

Explain the physical significance of Van der Waals parameters.

#### Critical temperature for carbon dioxide and methane are 31.1°C and – 81.9°C respectively.

Critical temperature for carbon dioxide and methane are 31.1°C and – 81.9°C respectively. Which of these has stronger intermolecular forces and why?

#### In terms of Charles’ law explain why -273°C is the lowest possible temperature.

In terms of Charles’ law explain why -273°C is the lowest possible temperature.

What would be the SI units for the quantity $$\dfrac{pV^2 T^2}{n}$$