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) The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr . (i) The pressure inside the tube due to the H2(g)

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Answer:

P (Hâ‚‚) = 741 torr

Explanation:

Let's begin by listing out the given parameters:

Temperature (water) = 298 K, volume = 45.6 mL,

atmospheric pressure, P (total) = 765 torr, vapor pressure of water, P (Hâ‚‚O) = 24 torr

To get the pressure of inside the tube, P (Hâ‚‚), we apply Dalton's Law of Partial Pressure and we have:

P (total) = P (Hâ‚‚) + P (Hâ‚‚O)

P (total) = 765 torr, P (Hâ‚‚O) = 24 torr

P (Hâ‚‚) = P (total) - P (Hâ‚‚O) = 765 - 24

P (Hâ‚‚) = 741 torr

It therefore becomes clear that the pressure of Hâ‚‚(g) is 741 torr

pstnonsonjoku

The pressure due to hydrogen is 741 torr.

According to Dalton's law of partial pressures, the total pressure of a gas mixture  is the sum of the partial pressures of all the individual gases in the mixture.

Total pressure of the gas = 765 torr

Vapor pressure of water = 24 torr

Pressure due to H2 = 765 torr - 24 torr  = 741 torr

Learn more about partial pressure: https://brainly.com/question/14623719

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