(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.

To learn more about Dalton Law follow the link:

link

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

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

the answer for sodium is 0.186

the answer for rubidium is 0.251