Question

If 4.65 LL of CO2CO2 gas at 22 ∘C∘C at 793 mmHg mmHg is used, what is the final volume, in liters, of the gas at 35 ∘C∘C and a pressure of 743 mmHg mmHg , if the amount of CO2CO2 does not change?

Answer 1

About 7.9 L.

Step-by-step explanation:

We can utilize the ideal gas law. Recall that:

`\displaystyle PV = nRT`

Because the amount of carbon dioxide does not change, we can rearrange to formula to:

`\displaystyle (PV)/(T)= nR`

Because the right-hand side stays constant, we have that:

`\displaystyle (P_1V_1)/(T_1) = (P_2V_2)/(T_2) = nR`

Hence substitute initial values and known final values:

`\displaystyle \begin{aligned} \frac{(793\text{ mm Hg})(4.65 \text{ L})}{(22 \text{ $^\circ$C})} & = \frac{(743 \text{ mm Hg})V_2}{(35\text{ $^\circ$C})} \\ \\ V_2 & = 7.9\text{ L}\end{aligned}`

Therefore, the final volume is about 7.9 L.