How many moles of chlorine gas and 120°c and 33.3 atm would occupy a vessel of 12 l?

The vessel contains 12.464 moles of chlorine gas.

To calculate the space occupied, we calculate the number of moles.

By ideal gas equation:

PV = nRT

P = pressure = 33.3 atm

V = volume = 12 L

n = moles

R = constant = 0.0816 l/atm/mol.K

T = temperature (K) = = + 273 = 393 K

n =

n =

n = 12.464 moles

The vessel contains 12.464 moles of chlorine gas.

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12.387 moles

We are given;

Temperature of chlorine, T = 120°C

But, K = °C + 273.15

Therefore, T = 393.15 K

Pressure, P = 33.3 Atm

Volume, V = 12 L

We are required to calculate the number of moles of chlorine gas,

To find the number of moles we are going to use the ideal gas equation;

PV = nRT

R is the ideal gas constant, 0.082057 L.atm/mol.K

Therefore, rearranging the formula;

n = PV÷RT

Hence;

n = (33.3 atm × 12 L) ÷ (0.082057 × 393.15 K)

  = 12.387 moles

Therefore, the number of moles of chlorine are 12.387 moles

c, liquids evaporate, creating a gas

2b2t

explanation:

2b2t