Question

If volume occupied by CO2 molecules is negligible,then the pressure exerted by one mole of CO2 gas in terms of temperature (T),assuming V to be single valued,is .....?

Answer 1

ANSWER:

The pressure will be 0.99 atm.

SOLUTION:

VOLUME = 22.4 liter;

NUMBER OF MOLES = 1.0 mole;

TEMPERATURE = 0 °C

a = 3.592 L2  atm/mol2

b = 0.04267 L/mol

We have the following assumptions:

1. Assume the ideal gas behavior.

2. Assume the non-ideal gas behavior (using Van der Waals)

Part 1: (ideal gas behavior)

R = 0.08206 L atm/mol K

using,

PV = nRT

P = nRT/V = (1.0 mol)(0.08206 L atm/mol K) (0+273)/(22.4 L)

P = 1.0 atm

Part 2:(non-ideal gas behavior)

According to the Van der Waal’s equation we have for one mole of a gas:

[P + a/V2] (V - b) = RT ….(1)

We have

R = 0.082 , T = 273K, V = 22.4 l for 1 mole of an ideal gas at 1 atm pressure.

[P + (3.592 L2 atm/mol2 ) (1.0 mol)2 /(22.4 L)2 ] [22.4 L – (1.0 mol)(0.04267 L/mol)] = (1.0 mol)(0.08206 L atm/mol K)(0+273 K)

P = 0.082 *273/22.4 – 3.592/(22.4)4

P=0.9922 atm

Answer 2

Answer:

DUDE ITS R²T²/4a

Look into attachment for details

Explanation:

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