How many moles of gas are present in the sample of gas occupies that 4.32 L at 1.45 atm pressure and -18oC? (Include your formula used and the set-up.)

The Ideal gas law states "that pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature of gas. It is expressed;

[tex]PV = nRT[/tex]

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

Given the data in the question;

Volume; [tex]V = 4.32L[/tex]

Pressure; [tex]P = 1.45atm[/tex]

Temperature; [tex]T = -18^oC = 255.15K[/tex]

Amount of gas; [tex]n =\ ?[/tex]

To determine the moles of gas, we substitute our given values into the expression above.

[tex]PV = nRT\\\\1.45atm * 4.32L = n * 0.08206Latm/molK * 255.15K\\\\6.264Latm = n * 20.937609Latm/mol\\\\n = \frac{6.264Latm}{20.937609Latm/mol} \\\\n = 0.3mol[/tex]

Therefore, the amount of gas present in the sample which occupied the given volume at the given pressure and temperature is 0.3mol.

Learn more about the Ideal gas law here: brainly.com/question/4147359