Question

What is the mass of silver (Ag) produced when 14.6 g of silver oxide (Ag₂O) undergoes the following reaction? Ag(s): 2Ag₂O(s) → 4Ag(s) + O₂(g)?

Answer 1

The mass of silver produced when 14.6 g of silver oxide undergoes the reaction is 21.87 g of silver.

Step-by-step explanation:

In the given reaction, 2 moles of silver oxide (Ag2O) produce 4 moles of silver (Ag). We can use this stoichiometry to find the mass of silver produced when 14.6 g of silver oxide undergoes the reaction.

First, we find the molar mass of Ag2O: Ag (107.87 g/mol) + O (16 g/mol) = 143.87 g/mol.

Next, we calculate the number of moles of Ag2O: 14.6 g Ag2O / 143.87 g/mol = 0.1014 mol Ag2O.

Finally, using the mole ratio from the balanced equation:

0.1014 mol Ag2O * (4 mol Ag / 2 mol Ag2O) = 0.2028 mol Ag.

Now, we can find the mass of Ag produced: 0.2028 mol Ag * 107.87 g/mol = 21.87 g of

Answer 2

The mass of silver (Ag) produced when 14.6 g of silver oxide (Ag₂O) undergoes the given reaction is 9.2 g.

Step-by-step explanation:

In the balanced chemical equation
`\(2Ag₂O(s) \rightarrow 4Ag(s) + O₂(g)\)`, it's evident that two moles of silver oxide (Ag₂O) yield four moles of silver (Ag). To find the molar mass of Ag₂O, we sum the atomic masses of silver (Ag) and oxygen (O). The molar mass of Ag₂O is
`\(2 * \text{atomic mass of Ag} + \text{atomic mass of O}\),` which equals
`\(2 * 107.87 + 15.9994 \, \text{g/mol} = 231.84 \, \text{g/mol}\).`

Now, we can calculate the moles of Ag₂O in 14.6 g using the formula:
`\(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\)`. Substituting the values, we get
`\(\frac{14.6 \, \text{g}}{231.84 \, \text{g/mol}} \approx 0.063 \, \text{moles}\)`. Since the mole ratio between Ag₂O and Ag is 1:2, the moles of silver formed is
`\(2 * 0.063 = 0.126 \, \text{moles}\).`

To find the mass of silver produced, we use the formula:
`\(\text{mass} = \text{moles} * \text{molar mass of Ag}\)`, giving us
`\(0.126 \, \text{moles} * 107.87 \, \text{g/mol} = 13.58 \, \text{g}\)`.

However, since not all the silver oxide is converted to silver, we must consider the limiting reactant. The limiting reactant is Ag₂O, and thus, the mass of silver produced is

`\(0.126 \, \text{moles} * 107.87 \, \text{g/mol} * 4 \, \text{(mole ratio)} = 9.2 \, \text{g}\).`