Hydrogen gas in 500cm^3 container at a pressure of 700 torr is transferred to a container of volume 700 cm^3. What will the new pressure be? a) if no temperature change occurs. b) if it's temperature changes from 25C to 35C?

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Hydrogen gas in 500cm^3 container at a pressure of 700 torr is transferred to a container of volume 700 cm^3. What will the new pressure be? a) if no temperature change occurs. b) if it's temperature changes from 25C to 35C?

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Answer 1 · 2017-04-23T13:58:41

Well, the combined gas law holds that $\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ $(P_1V_1)/T_1=(P_2V_2)/T_2$ , so..................

Explanation:

So we solve for $P_{2}$ $P_2$ , and thus $P_{2} = \frac{P_{1} V_{1}}{T_{1}} \times \frac{T_{2}}{V_{2}}$ $P_2=(P_1V_1)/T_1xxT_2/V_2$ , which clearly has the required units of pressure; why?

$P_2=(500*cancel(cm^3)xx700*"Torr")/(700*cancel(cm^3))=500*"Torr"$

The beauty of using these gas laws, is that (excluding temperature) given the proportionality, we can use whatever outlandish units we want, i.e. $"pounds per square inch, pints, furlongs"^3$ .

And for part (b), we must use units of $"absolute temperature"$ , $T_1=298*K; T_2=308*K$ :

$P_2=(700*"Torr"*500*cm^3)/(298*K)xx(308*K)/(700*cm^3)$ ,

$=517*"mm Hg"$

What are these pressure in $"atmospheres"$ ?

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Hydrogen gas in 500cm^3 container at a pressure of 700 torr is transferred to a container of volume 700 cm^3. What will the new pressure be? a) if no temperature change occurs. b) if it's temperature changes from 25C to 35C?

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Explanation:

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