The mass of HgO needed for the reaction is 216 g
The correct answer to the question is Option C. 216 g
We'll begin by calculating the theoretical yield of Hg.
- Actual yield of Hg = 100 g
- Theoretical yield of Hg =?
Theoretical yield = Actual yield / percentage yield
Theoretical yield = 100 / 50%
Theoretical yield of Hg = 200 g
Finally, we shall determine the mass of HgO needed for the reaction.
2HgO → 2Hg + O₂
Molar mass of HgO = 201 + 16 = 217 g/mol
Mass of HgO from the balanced equation = 2 × 217 = 434 g
Molar mass of Hg = 201 g/mol
Mass of Hg from the balanced equation = 2 × 201 = 402 g
From the balanced equation above,
402 g of Hg were produced from 434 g of HgO.
Therefore
200 g of Hg will be produce by = (200 × 434) / 402 = 216 g of HgO.
Thus, 216 g of HgO is needed for the reaction.
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