A 44.9-g sample of Ne gas exerts a certain pressure in a container of fixed volume. The mass of Ar is required to exert half the pressure at the same conditions of volume and temperature is 44.6 g.
given that :
mass of Ne = 44.9 g
moles of Ne = mass / molar mass
= 44.9 / 20
= 2.24 mol
using ideal gas equation we get :
P V = n RT
where,
volume V = constant
R = constant
T = temperature
therefore :
P1 / n1 = P2 / n2
P2 = P1 / 2
P1 / n1 = (P1 / 2 ) / n2
n2 = 2.24 / 2
= 1.12 mol
Mass of Ar = moles × molar mass
= 1.12 × 39.9
= 44.6 g.
Thus, A 44.9-g sample of Ne gas exerts a certain pressure in a container of fixed volume. The mass of Ar is required to exert half the pressure at the same conditions of volume and temperature is 44.6 g.
To learn more about ideal gas equation here
https://brainly.com/question/28837405
#SPJ4
