<u>Answer:</u> The value of
is coming out to be 0.412
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For
</u>
Given mass of
= 1.00 kg = 1000 g (Conversion factor: 1 kg = 1000 g)
Molar mass of
= 339.7 g/mol
Putting values in equation 1, we get:

Given mass of hydrogen gas = 10.0 g
Molar mass of hydrogen gas = 2 g/mol
Putting values in equation 1, we get:

- <u>For hydrogen sulfide:</u>
Given mass of hydrogen sulfide = 72.6 g
Molar mass of hydrogen sulfide = 34 g/mol
Putting values in equation 1, we get:

The chemical equation for the reaction of antimony sulfide and hydrogen gas follows:

Initial: 2.944 5
At eqllm: 2.944-x 5-3x 2x 3x
We are given:
Equilibrium moles of hydrogen sulfide = 2.135 moles
Calculating for 'x', we get:

Equilibrium moles of hydrogen gas = (5 - 3x) = (5 - 3(0.712)) = 2.868 moles
Volume of the container = 25.0 L
Molarity of a solution is calculated by using the formula:

The expression of
for above equation, we get:
![K_c=\frac{[H_2S]^3}{[H_2]^3}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BH_2S%5D%5E3%7D%7B%5BH_2%5D%5E3%7D)
The concentration of solids and liquids are not taken in the expression of equilibrium constant.

Hence, the value of
is coming out to be 0.412