If 1.00 x 1022 molecules of CO₂ gas are dissolved in 150.0 mL of aqueous solution,what is the STP volume of carbon dioxide dissolved in solution?

Question

Quizplus · Accepted Answer

To find the STP volume of carbon dioxide dissolved in solution, we use the ideal gas law and Avogadro's number. At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 L. Given 1.00 x 10^22 molecules of CO₂, we first convert molecules to moles using Avogadro's number (6.022 x 10^23 molecules/mol):$$ \text{Moles of CO}_2 = \frac{1.00 \times 10^{22} \text{ molecules}}{6.022 \times 10^{23} \text{ molecules/mol}} = 0.0166 \text{ mol} $$Then, to find the volume at STP, we multiply the moles by the volume occupied by one mole of gas at STP:$$ \text{Volume at STP} = 0.0166 \text{ mol} \times 22.4 \text{ L/mol} = 0.372 \text{ L} $$Therefore, the STP volume of carbon dioxide dissolved in the solution is 0.372 L.

If 100 X 1022 Molecules of CO₂ Gas Are Dissolved in in 150.0