Question

At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 kPa?

Answer 1

For this question, we will be using the Ideal gas Law formula, which is the following:

PV = nRT

Where:

P = pressure

V = volume

n = number of moles

R = constant of gases

T = temperature

We have:

P = 1.95 kPa or 0.019 atm

V = 12.30 L

n = 0.654 moles

R = 0.082 (this is an experimental value)

T = ?

Now we add these values into our formula:

0.019 * 12.30 = 0.654 * 0.082 * T

0.2337 = 0.0536T

T = 4.36 K