Question

Calculate the volume occupied by 2.59 mol of helium gas at a pressure of 0.826 atm and a temperature of 356 k.

Answer 1

The volume occupied by the given mol of helium gas at the given temperature and pressure is 91.6L.

Given the data in the question;

• Amount of helium; $n = 2.59mol$

• Pressure; $P = 0.826atm$

• Temperature; $T = 356K$

Volume of helium; $V = \ ?$

Ideal Gas Law

The Ideal gas law or general gas equation emphasizes on the state or behavior of a hypothetical ideal gas. It states that  pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature. It is expressed;

$PV = nRT$

Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant (  $R = 0.08206Latm/molK$ )

To determine the volume occupied by the helium gas, we substitute our values into the expression above.

$PV = nRT\\\\V = \frac{nRT}{P} \\\\V = \frac{2.59mol\ *\ 0.08206Latm/molK\ *\ 356K}{0.826atm} \\\\V = \frac{75.6626L}{0.826}\\ \\V = 91.6L$

Therefore, the volume occupied by the given mol of helium gas at the given temperature and pressure is 91.6L.

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