Question

What volume does 1.70 ×10–3 mol of chlorine gas occupy if its temperature is 20.2 °C and its pressure is 795 mm Hg?

Answer 1

Step-by-step explanation:

The given data is as follows.

No. of moles =
`1.70 * 10^(-3)`, V = ?

T = 20.2 + 273 K = 293.2 K, P =
`(795 mm Hg)/(760.0 mm Hg/atm)` = 1.046 atm, R =
`0.0821 L atm K^(-1)mol ^(-1)`

Calculate the volume using ideal gas equation as follows.

P V = n R T

`1.046 atm * V = 1.70 * 10^(-3) * 0.0821 L atm K^(-1)mol ^(-1) * 293.2 K`

V =
`(1.70 * 10^(-3) * 0.0821 L atm K^(-1)mol ^(-1) * 293.2 K)/(1.046 atm)`

=
`(40.921 L atm)/(1.046 atm)`

=
`39.122 * 10^(-3)` L

Thus, we can conclude that volume of the gas is
`39.122 * 10^(-3)` L.