A certain quantity of neon gas is under 1.05 atm pressure at 303 K in a 10.0 L vessel. How many moles of neon are present in the neon gas?
A) 0.222 mol
B) 0.402 mol
C) 0.422 mol
D) 2.37 mol

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the number of moles of neon present:

PV = nRT

where P is the pressure in atm, V is the volume in L, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Rearranging to solve for n, we get:

n = PV/RT

Plugging in the values given:

n = (1.05 atm)(10.0 L)/(0.0821 L·atm/mol·K)(303 K)

n = 0.422 mol

A Certain Quantity of Neon Gas Is Under 1