Question

In: Chemistry

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

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

Expert Solution

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

queen_honey_blossom answered 2 years ago

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