<u>Answer:</u> The mass of mercury (II) sulfide is 53.51 g
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For mercury (II) nitrate:</u>
Given mass of mercury (II) nitrate = 126.27 g
Molar mass of mercury (II) nitrate = 324.7 g/mol
Putting values in equation 1, we get:
- <u>For sodium sulfide:</u>
Given mass of sodium sulfide = 17.796 g
Molar mass of sodium sulfide = 78.04 g/mol
Putting values in equation 1, we get:
The chemical equation for the reaction of Mercury (II) nitrate and sodium sulfide follows:
By Stoichiometry of the reaction:
1 mole of sodium sulfide reacts with 1 mole of mercury (II) nitrate
So, 0.23 moles of sodium sulfide will react with = of mercury (II) nitrate
As, given amount of mercury (II) nitrate is more than the required amount. So, it is considered as an excess reagent.
Thus, sodium sulfide is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
1 mole of sodium sulfide produces 1 mole of mercury (II) sulfide
So, 0.23 moles of sodium sulfide will produce = of mercury (II) sulfide
Now, calculating the mass of mercury (II) sulfide from equation 1, we get:
Molar mass of mercury (II) sulfide = 232.66 g/mol
Moles of mercury (II) sulfide = 0.23 moles
Putting values in equation 1, we get:
Hence, the mass of mercury (II) sulfide is 53.51 g