# Problem: Calculate the mass (g) of each product formed when 174 g of silver sulfide reacts with excess hydrochloric acid: Ag2S(s) + HCl(aq) ⟶AgCl(s) + H2S(g) [unbalanced]

###### FREE Expert Solution

For this problem, we are being asked to calculate the mass of each product when 175 g silver sulfide is reacted with excess hydrochloric acid.

Step 1. Balance the equation:

Ag2S(s) + 2 HCl(aq)  2 AgCl(s) + H2S(g)

Step 2. Calculate the mass of AgCl and H2S.

Ag2S       2 Ag × 107.87 g/mol Ag = 215.74 g/mol
1 S × 32.06 g/mol S = 32.06 g/mol
Sum
247.8 g/mol

AgCl       1 Ag × 107.87 g/mol Ag = 107.87 g/mol
1 Cl × 35.45 g/mol Cl = 35.45 g/mol
Sum
143.3 g/mol

89% (248 ratings) ###### Problem Details

Calculate the mass (g) of each product formed when 174 g of silver sulfide reacts with excess hydrochloric acid: Ag2S(s) + HCl(aq) ⟶AgCl(s) + H2S(g) [unbalanced]

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Stoichiometry concept. You can view video lessons to learn Stoichiometry. Or if you need more Stoichiometry practice, you can also practice Stoichiometry practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Bracher's class at SLU.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.