Calculate the volume occupies by 0.125 mole of oxygen at 27⁰c and a pressure of 2.02×10⁵Nm-² [1 mole of gas occupies 22.4dm³ at S.T.P = 1.01×10⁵Nm-²]

PRESSURE: atmospheres or mm Hg; 1 atm = 760 mm Hg

TEMPERATURE: Kelvin, K, which is o

C + 273

STP: Standard Temperature and Pressure: 273 K and 1 atm (or 760 mm Hg)

BOYLE'S LAW (temperature is constant): PV = constant

This is an inverse relationship: if one variable increases the other must

decrease.

CHARLES' LAW (pressure is constant): V = constant x T

This is a direct relationship: if one variable increases so does the other.

GAY-LUSSAC'S LAW (volume is constant): P = constant x T

This is a direct relationship: if one variable increases so does the other.

IDEAL GAS LAW: PV = nRT, where

P = pressure of the gas

Explanation:

Look to the table of molar entropies provided to you.. Find the molar entropy, S for each compound at it's physical state in the reaction. Multiply by the number in the reaction, sum the products and reactants.

ΔS = S(products) - S(reactants)
ΔS = 2×(molEntropy of SO3 gas) - [2×(molEntropy of S solid) + 3×(molEntropy of O2 gas)]