Question

Imagine that the gas shown in the simulation is an ideal gas such as helium. Notice that the final number of moles of gas is 1.00 mol for each experimental run. You can find the final volume of the gas using they axis of the graph shown. Consider an experimental run at 273 K where the initial number of moles (n_i) is actually 1.00 mol, and the final number of moles (n_2) is 2.00 mol. Use the simulation to find the volume (V_1) of 1.00 mol of helium at 273 K, and calculate the final volume (V_2). Express the volume to three significant figures, and include the appropriate units.

Answer 1

For an ideal gas , PV=nRT

Or,V=nRT/P

Where,R=universal gas constant=0.0821 L atm K-1 mol-1)

T=temperature

(standard temp=273K)

P=pressure (std P=1 atm)

N= number of moles

V1=n1RT/P=(1.00 mol)* RT/P

V2=n2RT/P=(2.00 mol)* RT/P

V1/V2=1/2

2V1=V2

Putting the values of P,R.T,

V1=n1RT/P=(1.00 mol)*(0.0821 L atm K-1 mol-1)*(273K)/1 atm=22.413L

V2=2*V1=2*22.41L=44.82 6L

V2=44.826L