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

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:

∴

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

P = 1.40 atm

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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

the temperature of the gas, in k, not celsius.

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.