Respuesta :
Answer:
a) Total Volume = 46.18 cm³
b) Mole[tex]_{fraction}[/tex] (He) = 0.8333
c) Mole[tex]_{fraction}[/tex] (Ne) = 0.1666
d) Partial Pressure P[tex]_{He}[/tex] = 2648.68 atm
e) Partial Pressure P[tex]_{Ne}[/tex] = 529.73 atm
f) total pressure of the new laser tube = 3178.41 atm
Explanation:
Given that;
height of of discharge tube h = 1.2 m = 1.2 × 100 = 120cm
diameter of the tube D = 7 mm = 0.7cm
Radius = D/2 = 0.7/2 = 0.35 cm
a) What is the total volume (cm³)?
Volume = πr²h
we substitute
Volume = π × (0.35)² × 120
Volume = 46.18 cm³
b) What is the mole fraction of He?
Mole fraction of Helium will be;
Mole[tex]_{fraction}[/tex] (He) = Moles of He / Total Moles ( He + Ne)
given that; 5 mol He and 1 mol Ne
Mole[tex]_{fraction}[/tex] (He) = 5 / ( 5 + 1 )
Mole[tex]_{fraction}[/tex] (He) = 5 / 6
Mole[tex]_{fraction}[/tex] (He) = 0.8333
c) What is the mole fraction of Ne?
Mole fraction of Neon will be;
Mole[tex]_{fraction}[/tex] (Ne) = Moles of Ne / Total Moles ( He + Ne)
given that; 5 mol He and 1 mol Ne
Mole[tex]_{fraction}[/tex] (Ne) = 1 / ( 5 + 1 )
Mole[tex]_{fraction}[/tex] (Ne) = 1 / 6
Mole[tex]_{fraction}[/tex] (Ne) = 0.1666
d) d. What is the partial pressure of He (in atm)?
using ideal gas equation;
P[tex]_{He}[/tex] = nRT/V
where n is number or amount of moles( 5 )
R is the universal gas constant ( 0.08205 L-atm.mol⁻¹K⁻¹
T is temperature ( 298.15 K)
And V is the volume; ( 46.18 cm³ = 46.18/1000 = 0.04618 L )
so we substitute
P[tex]_{He}[/tex] = (5 × 0.08205 × 298.15) / 0.04618
P[tex]_{He}[/tex] = 122.316 / 0.04618
P[tex]_{He}[/tex] = 2648.68 atm
e) What is the partial pressure of Ne (in atm)?
P[tex]_{Ne}[/tex] = (1 × 0.08205 × 298.15) / 0.04618
P[tex]_{Ne}[/tex] = 24.463 / 0.04618
P[tex]_{Ne}[/tex] = 529.73 atm
f) What is the total pressure of the new laser tube (in atm)?
total pressure of the new laser tube will be;
= P[tex]_{He}[/tex] + P[tex]_{Ne}[/tex]
= 2648.68 atm + 529.73 atm
= 3178.41 atm
total pressure of the new laser tube = 3178.41 atm