Use the chemical equation to answer the question. 2Ag(s) + H2S(g) – Ag2S(s) + H2(g) The molar mass of silver (Ag) is 108 g/mol. The molar mass of sulfur (S) is 32 g/mol. The reaction uses 0.04 mol of silver. Which steps show how to determine the mass of silver sulfide (Ag2S) produced in the reaction?
108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.04 mol)=6.88 g
2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.04 mol)=9.92 g
2(108 g/mol)+32 g/mol=248 g/mol; (248 g/mol)(0.04 mol)(1 mol Ag2S / 2mol Ag)=4.96 g
108 g/mol+2(32 g/mol)=172 g/mol; (172 g/mol)(0.04 mol)(1 mol Ag2S/
2molAg)=3.44 g
I honestly don’t even know where to start.
This is a stoichiometry problem. Follow this four-step procedure to work all stoichiometry problems. If it is a limiting reagent problem it will work those, too, AFTER the limiting reagent has been determined. First off this is not a very practical problem; however, let's let that go and just solve the problem as if it can be easily done.
Step 1. Write and balance the equation.
2Ag(s) + H2S(g) ==> Ag2S + H2
Step 2. Determine moles of what you have. That usually is moles = grams/molar mass; however, that is already done and the problem tells you mols Ag = 0.04 moles.
Step 3. Using the coefficients in the balanced equation, convert mols of what you have (in this case it is moles Ag) into moles of what you want (in this case you want Ag2S).
0.04 mols Ag x (1 mol Ag2S/2 mols Ag) = 0.04 x 1/2 = 0.02 mols Ag2S
Step 4. Convert moles of what you want to grams (usually) or whatever.
grams Ag2S = moles Ag2S x molar mass Ag2S. The molar mass Ag2S = 2*108 + 32 = 248. Can you take this and fit it into one of the answers. My first suggestion is to work the problem using my steps and use that answer to eliminate wrong answers from the choices. I'll check back Stay in tough if you still have questions.
To determine the mass of silver sulfide (Ag2S) produced in the reaction, you need to use the given molar mass of silver (Ag) and sulfur (S) and the stoichiometry of the balanced equation.
Let's break down the steps:
Step 1: Find the molar mass of Ag2S
The molar mass of Ag2S can be calculated by summing the atomic masses of its constituent atoms. Since each mole of Ag has a molar mass of 108 g/mol and each mole of S has a molar mass of 32 g/mol, the molar mass of Ag2S is calculated as follows:
Molar mass of Ag2S = 2(108 g/mol) + 32 g/mol = 248 g/mol
Step 2: Calculate the moles of Ag used in the reaction
The given amount of Ag used in the reaction is 0.04 mol.
Step 3: Determine the moles of Ag2S produced
Using the stoichiometry of the balanced equation, we can see that 2 moles of Ag react to form 1 mole of Ag2S. Therefore, for every 2 moles of Ag used, 1 mole of Ag2S is produced.
So, we can convert the moles of Ag used (0.04 mol) to moles of Ag2S produced as follows:
Moles of Ag2S = 0.04 mol × (1 mol Ag2S/2 mol Ag)
Moles of Ag2S = 0.02 mol Ag2S
Step 4: Calculate the mass of Ag2S produced
Lastly, we can convert the moles of Ag2S produced to grams using its molar mass calculated in Step 1:
Mass of Ag2S = Moles of Ag2S × Molar mass of Ag2S
Mass of Ag2S = 0.02 mol × 248 g/mol = 4.96 g
Therefore, the correct answer is:
2(108 g/mol) + 32 g/mol = 248 g/mol; (248 g/mol)(0.04 mol)(1 mol Ag2S/2 mol Ag) = 4.96 g
To determine the mass of silver sulfide (Ag2S) produced in the reaction, we need to use the given molar mass of silver (Ag) and the balanced chemical equation.
Step 1: Calculate the molar mass of Ag2S:
The molar mass of Ag2S can be calculated by adding the molar masses of Ag and S. Since there are two Ag atoms in Ag2S, we multiply the molar mass of Ag by 2 and add it to the molar mass of S.
Molar mass of Ag = 108 g/mol
Molar mass of S = 32 g/mol
Molar mass of Ag2S = 2(108 g/mol) + 32 g/mol = 248 g/mol
Step 2: Calculate the moles of Ag used in the reaction:
The given information states that the reaction uses 0.04 mol of silver (Ag).
Step 3: Convert moles of Ag to moles of Ag2S:
To convert the moles of Ag to moles of Ag2S, we need to use the stoichiometric ratio in the balanced chemical equation. The coefficient of Ag2S is 1, and the coefficient of Ag is 2.
Moles of Ag2S = (0.04 mol Ag) * (1 mol Ag2S / 2 mol Ag) = 0.02 mol Ag2S
Step 4: Calculate the mass of Ag2S produced:
To determine the mass of Ag2S, multiply the moles of Ag2S by its molar mass calculated in Step 1.
Mass of Ag2S = (0.02 mol Ag2S) * (248 g/mol) = 4.96 g
Therefore, the correct answer is:
(248 g/mol)(0.04 mol)(1 mol Ag2S / 2 mol Ag) = 4.96 g