Question

A 4.00g sample of helium has a volume of 24.4L at a temperature of 25.0 C and a pressure of 1.00 atm. The volume of the helium is reduced to 10.4L, but the temperature and pressure of the gas are kept constant. What is the new quantity of the gas in moles

Answer 1

0.852 mol

Step-by-step explanation:

First we convert 4.00 g of helium (He) into moles, using its molar mass:

4.00 g ÷ 2 g/mol = 2 mol He

To answer this problem we can use Avogadro's law, which states that at constant pressure and temperature:

V₁n₂=V₂n₁

Where:

• V₁ = 24. 4 L

• n₂ = ?

• V₂ = 10.4 L

• n₁ = 2 mol

We input the data:

• 24.4 L * n₂ = 10.4 L * 2 mol

And solve for n₂:

• n₂ = 0.852 mol