Question

Chloroform, CHCI3, is a volatile (easily vapourised) liquid solvent. Calculate the density of chloroform vapour at 99 Cand 745 mmHg. Give the answer in gram per litre.
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Answer 1

Answer:hope it helps

Mark

Explanation:PV = nRT

You know P. Assume V = 1 L. You know R and T. Calculate n = mols and that is mols in 1 L.

mols = g/molar mass. you now know mols and you know molar mass. Calculate grams. And that is in 1 L so the answer is g/L. You can do it another way all in one step if you want to redo the equation a little.

PV = nRT

P = (n/V)*RT

but n = g/molar mass so

P = (g/molar mass*V)*RT

But g/V = density = d so

P = (d/molar mass)*RT and solve for d.

d = (P*molar mass)/(RT)

Answer 2

Answer:

3.83 g / L

Explanation:

Given :

Temperature = 99 C

In term of Kelvin

T = 99 + 273 K

T = 372 K

Pressure in term of atm

P = 745 / 760 atm

P = 0.98 atm

We have density formula i.e.

d = P M / R T

where M is molar mass and R is universal gas constant .

R = 0.0821 L atm / mol

Molar mass of Chloroform CHCl₃ = 119.5 g / mol

Putting value in formula of d

d = ( 0.98 × 119.5 ) / ( 0.0821 × 372 ) g / L

d = 3.83 g / L

Therefore , density of chloroform is 3.83 g / L .