Question

Find Density of CO2 at 127 Degree Celsius & 2 ATM Pressure.

Answer 1

Answer:

T=27⁰C =27+273=300K

P =2.5 atm

The molar mass of (M) CO2 =44g/mol

from ideal gas equation,

d =PM / RT =2.5×44 / 0.0821 ×300 = 4.46g L‐¹

Explanation:

PLEASE MARK IT At BRAINLIST

Answer 2

Answer:

The density of $CO_{2}$ is 2.67 g/L.

Explanation:

Given:

Temperature=127°C = 127°C + 273.15 = 400.15K

Pressure = 2 ATM

The molar mass of $CO_{2}$ = (12)+(2x16)= 44g/mol

R=0.0821

Density=$\frac{PM}{RT}$

Where P is pressure , M is molar mass, R is constant and T is temperature .

Now substituting the values in the formula,

density= $\frac{2*44}{0.0821 * 400.15}$

density= $\frac{88}{32.85}$

density= 2.67 g/L

#SPJ2