Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 decade ago

# What is the density of carbon tetrachloride vapor at STP?

How do I find the density of carbon tetrachloride vapor at STP?

Relevance
• Anonymous

STP means standard temperature and pressure

T = 273 K

P = 1 atm

We need to find the density = (mass / volume)

We can find the volume of the gas if we use the ideal gas law

(pressure) x (volume) = (# of moles) x (temperature) x R

V = (n x T x R) / (P)

Because density is an intensive property (it does not change with the amount), we will assume one mole of CCl4

So now

P = 1 atm

T = 273 K

n = 1 mole

R = 0.0821 (L*atm) / (Mole *K)

V = (1 mole x 273 K x 0.0821((L*atm)/(mole*K))) / (1 atm) = 22.4 L

This volume is expected with STP of any ideal gas

Now we need mass. We assumed 1 mole of CCl4 to find the volume, so we find the mass of 1 mole of CCl4

1 mole CCl4 x (154 g/mol) = 154 g CCl4

Now we solve for density

D = m/V = 154 g/22.4 L = 6.875 g/L

0.006875 g/ mL

http://www.emerico.com

• Anonymous
4 years ago

Density Of Carbon Tetrachloride

• 1 decade ago

Molar mass CCl4 = 153.8236 g/mol

this mass of vapour has volume of 22.4 litres at STP

Mass of 1 litre at STP = 153.8236/22.4 = 6.86g/litre

Answer: Density of CCl4 gas at STP = 6.86g/litre.