(d) In the laboratory, the temperature is 295 K and the total pressure in the gas-collecting tube is 741.2 mmHg . If the vapor pressure of water at 295 K is 19.8 mmHg , determine the pressure of the H2(g) in the gas-collecting tube.

According to the Dalton Law in a blend of non-reacting gases, the entire pressure will be equivalent to the total of partial pressures of the individual gases.

The pressure of H₂ gas collected in the tube will be 721.3 mm Hg.

This can be calculated by:

Dalton's formula:

Given :  

Now using the formula we will calculate:

Therefore, the pressure of the hydrogen in the tube is 721.3 mm Hg.

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The pressure of the hydrogen in the gas-collecting tube is 721.3 mm Hg

Explanation:

According to Dalton's law, the total pressure is the sum of individual pressures.

Given : =total pressure of gases = 741.1 mm Hg

= partial pressure of water = 19.8 mm Hg

= partial pressure of hydrogen = ?

putting in the values we get:

Thus  the pressure of the hydrogen in the gas-collecting tube is 721.3 mm Hg

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the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.