Question

the density of carbon dioxide is equal to 1.965 kg m ^-3 at 273K And 1 atm pressure ​

Answer 1

Answer:

Your solution is in the picture

Answer 2

Explanation:

Final Answer : Molar Mass of CO2 = 44.042g

Assuming gas is Ideal :

Steps and Understanding :

1) Given,

Temperature , T = 273K

Pressure, P = 1atm

Density, d = 1.965 kg/m^3 = 1.965g/L

Gas Constant, R = 0.0821 Latm /K/mole

2)

Let Molar Mass of CO2 be M g.

Then,

Equation :

d = PM/RT

=>

\begin{lgathered}1 .965 = \frac{1 \times m}{0.0821 \times 273} \\ = > m = 0.0821 \times 273 \times 1.965 \\ = > m = 44.042 \: g \:\end{lgathered}1.965=0.0821×2731×m=>m=0.0821×273×1.965=>m=44.042g

Therefore, Molar Mass of CO2 is 44.042g.