Question

A 5.3 L volume of ideal neon gas (monatomic) is at a pressure of 6.0 atmospheres and a temperature of 290 K. The atomic mass of neon is 20.2 g/mol. For problems with these units, if you use the gas constant R = 0.0821 (L atm)/(mol K), you won't have to do a lot of unit conversion of the rest of the quantities given. The mass of the neon gas, in SI units, is closest to:
A) 2.7 × 10^1
B) 2.7 × 10^3
C) 2.7 × 10^-2
D) 1.6 × 10^-2
E) 1.3 × 10^1

Answer 1

Volume of the sample of the ideal gas,V =5.3 L

Pressure,P =6 atm

Temperature,T =290 K

Gas constant,R =  0.0821 L-atm/K-mol.

Atomic mass of the neon ,M =20.2 g/mol.

Calculate the  mass of the neon by using the ideal gas equation.

PV =m(R/M )T

m= PVM/RT

m =(6)(5.3)(20.2)/(0.0821)(290)

   =27 g

   =2.7×10¹

Therefore, the  option A is correct.