Question

How much pressure would 0.8 moles of a gas at 370K exert if it occupied 17.3L of space

Answer 1

Answer:

1.40 atm is the pressure for the gas

Explanation:

An easy problem to solve with the Ideal Gases Law:

P . V = n . R .T

T° = 370K

V = 17.3L

n = 0.8 mol

Let's replace data → P . 17.3L = 0.8mol . 0.082L.atm/mol.K . 370K

P = (0.8mol . 0.082L.atm/mol.K . 370K) / 17.3L = 1.40 atm

Answer 2

The amount of pressure needed to be exerted is 1.40 atm.

The ideal gas equation shows the relation between the number of moles of a given gaseous substance, its volume, pressure, and temperature.

It can be expressed by using the formula:

PV = nRT

From the parameters given:

• The number of moles n = 0.8
• The temperature of the gas = 370 K
• The volume of the gas occupied in space = 17.3 L
• The gas rate constant R = 0.082 L.atm/mol.K

∴

Making the pressure the subject of the formula from the above equation, we have:

$\mathbf{P = \dfrac{nRT}{V}}$

$\mathbf{P = \dfrac{0.8 \times 0.082 \times 370}{17.3}}$

P = 1.40 atm

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