What volume will 500 mL of gas at 20°C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80°C and the pressure is increased to 650 mm Hg?

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What volume will 500 mL of gas at 20°C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80°C and the pressure is increased to 650 mm Hg?

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Answer 1 · 2018-07-27T05:17:15

Approx. $200 \cdot m L$ $200*mL$ ...…...

Explanation:

The combined gas law holds that $\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $(P_1V_1)/T_1=(P_2V_2)/T_2$ ...we use terms of absolute temperature...we also KNOW that $1 \cdot a t m$ $1*atm$ will support a column of mercury that is $760 \cdot m m$ $760*mm$ high...

And so we solve for... $V_{2} = \frac{P_{1} V_{1}}{T_{1}} \times \frac{T_{2}}{P_{2}}$ $V_2=(P_1V_1)/T_1xxT_2/P_2$

$= \frac{\frac{420 \cdot m m \cdot H g}{760 \cdot m m \cdot a t m^{- 1}} \cdot 500 \cdot m L}{293.15 \cdot K} \times \frac{193.15 \cdot K}{\frac{650 \cdot m m \cdot H g}{760 \cdot m m \cdot a t m^{- 1}}}$ $=((420*mm*Hg)/(760*mm*atm^-1)*500*mL)/(293.15*K)xx(193.15*K)/((650*mm*Hg)/(760*mm*atm^-1))$

$= ? ? \cdot m L$ $=??*mL$

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What volume will 500 mL of gas at 20°C and a pressure of 420 mm Hg occupy if the temperature is reduced to -80°C and the pressure is increased to 650 mm Hg?

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Explanation:

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