Answer:
34g
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
H2S + 2AgNO3 —> 2HNO3 + Ag2S
Next, we shall determine the number of mole of H2S required to react with 2 moles of AgNO3.
This is illustrated below:
From the balanced equation above,
We can see that 1 mole of H2S is required to react completely with 2 moles of AgNO3.
Finally, we shall convert 1 mole of H2S to grams. This is shown below:
Number of mole H2S = 1 mole
Molar mass of H2S = (2x1) + 32 = 34g/mol
Mass = number of mole x molar Mass
Mass of H2S = 1 x 34
Mass of H2S = 34g
Therefore, 34g of H2S is needed to react with 2 moles of AgNO3.
Molar mass is the mass of one mole of the substance.The mass of the Hydrogen sulfide in the given reaction is 34 g.
Molar mass:
It is the mass of one mole of the substance. Molar mass of a compound is the sum of atomic mass of their constituent elements.
Here,
Atomic mass of hydrogen = 1
Atomic mass of the Sulfur = 32
So, molar mass of the the Hydrogen sulfide([tex]\bold {H_2S}[/tex])
= 2(1 )+ 32
= 2+32
= 34
The given reaction,
[tex]\bold {H2_S + 2AgNO_3 \rightarrow 2HNO_3 + Ag2_S}[/tex]
1 mole of hydrogen sulfide react with 2 moles of silver nitrate to form 2 moles of nitric acid and one mole of silver sulfate.
Since, in the reaction only one mole of Hydrogen sulfide is consumed..
Therefore, the mass of the Hydrogen sulfide in the given reaction is 34 g.
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