Question

A sample of hydrogen gas collected by displacement of water occupied 30.0 mL at 24oC on a day when the barometric pressure was 736 torr. What volume would the hydrogen occupy if it were dry and at STP? The vapor pressure of water at 24.0oC is 22.4 torr.

I know it needs the combined gas law but further elaboration would be useful

Answer 1

Explanation:

like it is simple calculation

+24-24.0+(-22.4)+(-736)+30

so your total answer is -788.4

hope help you

...

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Answer 2

Concept

Barometric pressure is an atmospheric pressure which is caused by the weight of the air

Given

• Initial volume of Hydrogen given is 30.0ml
• The temperature given is 24°C
• The barometric pressure given is 736 torr
• The vapor pressure of water given is 22.4 torr

Find

We need to find the volume of the Dry hydrogen at STP

Solution

By using the combined gas law

$\frac{P_1V_1}{T_1}= \frac{P_2V_2}{T_2}$

∴$\frac{736*30}{297} = \frac{760*V_2}{273}$

$V_2=\frac{736*30*273}{297*760}\\=26.7ml$

Hence the volume of dry hydrogen is 26.7ml

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