If a sample of helium gas at 870 torr and 22 degrees C is allowed to expand from 23 L to 55 L without changing the temperature, what pressure will the helium gas exert?

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If a sample of helium gas at 870 torr and 22 degrees C is allowed to expand from 23 L to 55 L without changing the temperature, what pressure will the helium gas exert?

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Answer 1 · 2018-05-25T17:57:41

Well, for a start...the measurement of pressure is illegitimate...

Explanation:

We know that one atmosphere will support a column of mercury that is $760 \cdot m m$ $760*mm$ high. A mercury column is thus a good measure for pressures at $1 \cdot a t m$ $1*atm$ or much LOWER than $1 \cdot a t m$ $1*atm$ ..

And so here $P = \frac{870 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}} = 1.15 \cdot a t m$ $P=(870*mm*Hg)/(760*mm*Hg*atm^-1)=1.15*atm$ .

And so $P_{1} V_{1} = P_{2} V_{2}$ $P_1V_1=P_2V_2$ ...and $P_{2} = \frac{P_{1} V_{1}}{V_{2}}$ $P_2=(P_1V_1)/V_2$

$= \frac{1.15 \cdot a t m \times 23 \cdot L}{55 \cdot L} = 0.479 \cdot a t m \equiv 363.8 \cdot m m \cdot H g$ $=(1.15*atmxx23*L)/(55*L)=0.479*atm-=363.8*mm*Hg$

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If a sample of helium gas at 870 torr and 22 degrees C is allowed to expand from 23 L to 55 L without changing the temperature, what pressure will the helium gas exert?

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