A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

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Answer 1 · 2017-06-12T09:55:50

$212$ $212$ $torr$ $"torr"$

$\Rightarrow \frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $Rightarrow frac(P_(1) V_(1))(T_(1)) = frac(P_(2) V_(2))(T_(2))$

In our case, the temperature of $125^{\circ}$ $125^(@)$ $C$ $"C"$ is kept constant throughout the process, so $T_{1} = T_{2}$ $T_(1) = T_(2)$ :

$\Rightarrow \frac{P_{1} V_{2}}{T_{1}} = \frac{P_{2} V_{2}}{T_{1}}$ $Rightarrow frac(P_(1) V_(2))(T_(1)) = frac(P_(2) V_(2))(T_(1))$

$\Rightarrow P_{1} V_{1} = P_{2} V_{2}$ $Rightarrow P_(1) V_(1) = P_(2) V_(2)$

Then, let's substitute the relevant values:

$\Rightarrow 248$ $Rightarrow 248$ $torr \times 275$ $"torr" times 275$ $L = P_{2} \times 321$ $"L" = P_(2) times 321$ $L$ $"L"$

$\Rightarrow P_{2} = \frac{248 torr \times 275 L}{321 L}$ $Rightarrow P_(2) = frac(248 " torr" times 275 " L")(321 " L")$

$therefore P_(2) = 212.46105919$ $"torr"$

Therefore, the final gas pressure will be around $212$ $"torr"$ .