Question

find the mass of h2 produced Binary compounds of alkali metals and hydrogen react with water to produce H2(g). The H2H2 from the reaction of a sample of NaH with an excess of water fills a volume of 0.505 L above the water. The temperature of the gas is 35 ∘C∘C and the total pressure is 755 mmHg

Answer 1

Answer: Mass of hydrogen produced is 0.0376 g.

Step-by-step explanation:

The reaction equation will be as follows.

`NaH(aq) + H_(2)O(l) \rightarrow H_(2)(g) + NaOH(aq)`

Now, formula for total pressure will be as follows.

`P_(total) = P_{H_(2)} + P_{H_(2)O}`

Hence,
`P_{H_(2)} = P_(total) - P_{H_(2)O}`

= 755 mm Hg - 42.23 mm Hg

= 712.77 mm Hg

`P_{H_(2)} = (712.77 * 1 atm)/(760 mm Hg)`

= 0.937 atm

Now, we will calculate the moles of
`H_(2)` as follows.

`P_{H_(2)}V = nRT`

`0.937 atm * 0.505 L = n * 0.0821 * 308.15 K`

n =
`(0.473)/(25.29)` mol

= 0.0187 mol

Therefore, mass of
`H_(2)` will be calculated as follows.

`m_{H_(2)} = (0.0187 mol * 2.0158 g)/(1 mol)`

= 0.0376 g

Thus, we can conclude that mass of hydrogen produced is 0.0376 g.