Sure, here are the steps to solve this problem:

1. First, we need to find out how much oxygen reacted with the silver. We can do this by subtracting the mass of the silver from the mass of the metal oxide. So, 8.55 g (metal oxide) - 7.96 g (silver) = 0.59 g of oxygen.

2. Next, we need to convert these masses into moles. We do this by dividing the mass of each element by its molar mass. So, for silver (Ag), we have 7.96 g ÷ 107.87 g/mole = 0.0738 moles. For oxygen (O), we have 0.59 g ÷ 16.00 g/mole = 0.0369 moles.

3. Now, we need to find the simplest whole number ratio of moles of silver to moles of oxygen. We do this by dividing each number of moles by the smallest number of moles. So, for silver, we have 0.0738 ÷ 0.0369 = 2. For oxygen, we have 0.0369 ÷ 0.0369 = 1.

4. Therefore, the formula of the oxide is Ag2O.

Question

Sure, here are the steps to solve this problem:

1. First, we need to find out how much oxygen reacted with the silver. We can do this by subtracting the mass of the silver from the mass of the metal oxide. So, 8.55 g (metal oxide) - 7.96 g (silver) = 0.59 g of oxygen.

2. Next, we need to convert these masses into moles. We do this by dividing the mass of each element by its molar mass. So, for silver (Ag), we have 7.96 g ÷ 107.87 g/mole = 0.0738 moles. For oxygen (O), we have 0.59 g ÷ 16.00 g/mole = 0.0369 moles.

3. Now, we need to find the simplest whole number ratio of moles of silver to moles of oxygen. We do this by dividing each number of moles by the smallest number of moles. So, for silver, we have 0.0738 ÷ 0.0369 = 2. For oxygen, we have 0.0369 ÷ 0.0369 = 1.

4. Therefore, the formula of the oxide is Ag2O.

Knowee AI · Accepted Answer

Sure, here are the steps to solve this problem:

1. First, we need to find out how much oxygen reacted with the silver. We can do this by subtracting the mass of the silver from the mass of the metal oxide. So, 8.55 g (metal oxide) - 7.96 g (silver) = 0.59 g of oxygen.

2. Next, we need to convert these masses into moles. We do this by dividing the mass of each element by its molar mass. So, for silver (Ag), we have 7.96 g ÷ 107.87 g/mole = 0.0738 moles. For oxygen (O), we have 0.59 g ÷ 16.00 g/mole = 0.0369 moles.

3. Now, we need to find the simplest whole number ratio of moles of silver to moles of oxygen. We do this by dividing each number of moles by the smallest number of moles. So, for silver, we have 0.0738 ÷ 0.0369 = 2. For oxygen, we have 0.0369 ÷ 0.0369 = 1.

4. Therefore, the formula of the oxide is Ag2O.

A 7.96 gram sample of silver reacts with oxygen to form 8.55 gram of the metal oxide. What is the formula of the oxide, given the following molar masses (Ag: 107.87 g/mole; O: 16.00 g/mole)?

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