Question

using the temperature of air, barometric pressure, and volume of flask, calculate moles of air for each trial.

trial 1: temperature of air: 20.1 deg Celcius, barometric pressure: 742.44 Hg, volume of flask: 285 ml

Trial 2: Temp of air 20.2 deg celcius. Barametric pressure: 742.44 Hg , volume : 285 ml

Answer 1

Trial 1 :

Use ideal gas equation for calculation of mole of gas

Ideal gas equation

PV = nRT             where, P = atm pressure= 742.44 mm Hg = 0.9769 atm,

V = volume in Liter = 285 ml = 0.285 L

n = number of mole = ?

R = 0.08205L atm mol^-1 K^-1 =Proportionality constant = gas constant,

T = Temperature in K = 20.1⁰C = 273.15+ 20.1 = 293.25 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.9769 0.285)/(0.08205 293.25) = 0.011571199 mole

0.011571199 mole of air

Trial 2 :

Use ideal gas equation for calculation of mole of gas

Ideal gas equation

PV = nRT             where, P = atm pressure= 742.44 mm Hg = 0.9769 atm,

V = volume in Liter = 285 ml = 0.285 L

n = number of mole = ?

R = 0.08205L atm mol^-1 K^-1 =Proportionality constant = gas constant,

T = Temperature in K = 20.2⁰C = 273.15+ 20.2 = 293.35 K

We can write ideal gas equation

n = PV/RT

Substitute the value

n = (0.9769 0.285)/(0.08205 293.35) = 0.0115672545 mole

0.0115672545 mole of air