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

Explanation:

The given data is as follows.

     No. of moles = $1.70 \times 10^{-3}$,           V = ?

     T = 20.2 + 273 K = 293.2 K,             P = $\frac{795 mm Hg}{760.0 mm Hg/atm}$ = 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

    $1.046 atm \times V = 1.70 \times 10^{-3} \times 0.0821 L atm K^{-1}mol ^{-1} \times 293.2 K$

                                  V = $\frac{1.70 \times 10^{-3} \times 0.0821 L atm K^{-1}mol ^{-1} \times 293.2 K}{1.046 atm}$

                                   = $\frac{40.921 L atm}{1.046 atm}$

                                   = $39.122 \times 10^{-3}$ L

Thus, we can conclude that volume of the gas is $39.122 \times 10^{-3}$ L.