calculate the mass of silver chloride and dihydrogen monosulfide formed when 85.6g of silver sulfide reacts with excess hydrochloric acid.

To calculate the mass of silver chloride and dihydrogen monosulfide formed when a reaction occurs, we need to understand the balanced chemical equation for the reaction between silver sulfide and hydrochloric acid.

The balanced chemical equation for the reaction is as follows:

Ag2S + 2HCl -> 2AgCl + H2S

From the equation, we can see that one mole of silver sulfide (Ag2S) reacts with two moles of hydrochloric acid (2HCl) to produce two moles of silver chloride (2AgCl) and one mole of dihydrogen monosulfide (H2S).

Now let's proceed with the calculation steps:

Step 1: Calculate the number of moles of silver sulfide (Ag2S) used.
To do this, we need to know the molar mass of silver sulfide (Ag2S). The molar mass of silver (Ag) is 107.87 g/mol, and the molar mass of sulfur (S) is 32.07 g/mol.
So, the molar mass of silver sulfide (Ag2S) is:
(2 x molar mass of Ag) + molar mass of S
= (2 x 107.87 g/mol) + 32.07 g/mol
= 243.81 g/mol

Moles of Ag2S = Mass of Ag2S / Molar mass of Ag2S
= 85.6 g / 243.81 g/mol
= 0.3513 mol of Ag2S (rounded to four decimal places)

Step 2: Determine the limiting reactant.
Since we have an excess of hydrochloric acid, the limiting reactant will be silver sulfide (Ag2S). This means that all of the Ag2S will be consumed in the reaction, and the amount of product formed will be determined by the amount of Ag2S.

Step 3: Calculate the moles of silver chloride (AgCl) and dihydrogen monosulfide (H2S) formed.
From the balanced equation, we see that 1 mole of Ag2S produces 2 moles of AgCl and 1 mole of H2S.
So, moles of AgCl formed = 2 x moles of Ag2S
= 2 x 0.3513 mol
= 0.7026 mol of AgCl

Moles of H2S formed = 1 x moles of Ag2S
= 1 x 0.3513 mol
= 0.3513 mol of H2S

Step 4: Calculate the mass of AgCl and H2S formed using their molar masses.
The molar mass of silver chloride (AgCl) is 143.32 g/mol, and the molar mass of dihydrogen monosulfide (H2S) is 34.08 g/mol.

Mass of AgCl = Moles of AgCl x Molar mass of AgCl
= 0.7026 mol x 143.32 g/mol
= 100.58 g of AgCl (rounded to two decimal places)

Mass of H2S = Moles of H2S x Molar mass of H2S
= 0.3513 mol x 34.08 g/mol
= 11.97 g of H2S (rounded to two decimal places)

Therefore, when 85.6 g of silver sulfide reacts with excess hydrochloric acid, approximately 100.58 g of silver chloride and 11.97 g of dihydrogen monosulfide are formed.

To calculate the mass of silver chloride and dihydrogen monosulfide formed when 85.6g of silver sulfide reacts with excess hydrochloric acid, we need to determine the balanced chemical equation for the reaction.

The balanced equation for the reaction between silver sulfide (Ag2S) and hydrochloric acid (HCl) is:

Ag2S + 2HCl → 2AgCl + H2S

From the balanced equation, we can see that 1 mole of silver sulfide produces 2 moles of silver chloride and 1 mole of dihydrogen monosulfide (hydrogen sulfide).

Step 1: Convert the given mass of Ag2S to moles.
To do this, we need to know the molar mass of Ag2S, which can be calculated as follows:

Molar mass of Ag = 107.87 g/mol
Molar mass of S = 32.07 g/mol

Molar mass of Ag2S = 2 x molar mass of Ag + molar mass of S
= (2 x 107.87 g/mol) + 32.07 g/mol
= 243.81 g/mol

To find the number of moles of Ag2S, we divide the given mass by its molar mass:
Number of moles of Ag2S = Mass of Ag2S / Molar mass of Ag2S
= 85.6 g / 243.81 g/mol
≈ 0.3513 mol (rounded to 4 decimal places)

Step 2: Calculate the moles of AgCl formed.
From the balanced equation, we can see that 1 mole of Ag2S produces 2 moles of AgCl.
So, the moles of AgCl formed will be twice the moles of Ag2S:
Moles of AgCl = 2 x Moles of Ag2S
= 2 x 0.3513 mol
= 0.7026 mol (rounded to 4 decimal places)

Step 3: Convert the moles of AgCl to mass.
To do this, we need to know the molar mass of AgCl, which can be calculated as follows:

Molar mass of Ag = 107.87 g/mol
Molar mass of Cl = 35.45 g/mol

Molar mass of AgCl = Molar mass of Ag + Molar mass of Cl
= 107.87 g/mol + 35.45 g/mol
= 143.32 g/mol

To find the mass of AgCl, we multiply the moles of AgCl by its molar mass:
Mass of AgCl = Moles of AgCl x Molar mass of AgCl
= 0.7026 mol x 143.32 g/mol
= 100.63 g (rounded to 2 decimal places)

Step 4: Calculate the moles of H2S formed.
From the balanced equation, we can see that 1 mole of Ag2S produces 1 mole of H2S.
So, the moles of H2S formed will be the same as the moles of Ag2S:
Moles of H2S = Moles of Ag2S = 0.3513 mol (rounded to 4 decimal places)

Step 5: Convert the moles of H2S to mass.
To do this, we need to know the molar mass of H2S, which can be calculated as follows:

Molar mass of H = 1.01 g/mol
Molar mass of S = 32.07 g/mol

Molar mass of H2S = 2 x Molar mass of H + Molar mass of S
= 2 x 1.01 g/mol + 32.07 g/mol
= 34.09 g/mol

To find the mass of H2S, we multiply the moles of H2S by its molar mass:
Mass of H2S = Moles of H2S × Molar mass of H2S
= 0.3513 mol × 34.09 g/mol
= 11.97 g (rounded to 2 decimal places)

Therefore, the mass of silver chloride formed is approximately 100.63 g, and the mass of dihydrogen monosulfide formed is approximately 11.97 g.

Here is an example problem. Just follow the steps.

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