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)? Group of answer choicesAgOAgO2Ag2OAg3Onone of the above.
Question
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)? Group of answer choicesAgOAgO2Ag2OAg3Onone of the above.
Solution
To find the formula of the oxide, we need to determine the amount of oxygen that reacted with the silver.
Step 1: Find the mass of oxygen Subtract the mass of the silver from the total mass of the metal oxide to find the mass of the oxygen. 8.55 g (total mass of metal oxide) - 7.96 g (mass of silver) = 0.59 g (mass of oxygen)
Step 2: Convert the mass of silver and oxygen to moles Divide the mass of each element by its molar mass to convert it to moles. Silver: 7.96 g ÷ 107.87 g/mole = 0.0738 moles Oxygen: 0.59 g ÷ 16.00 g/mole = 0.0369 moles
Step 3: Find the ratio of moles of silver to moles of oxygen Divide the number of moles of each element by the smallest number of moles calculated. Silver: 0.0738 moles ÷ 0.0369 moles = 2 Oxygen: 0.0369 moles ÷ 0.0369 moles = 1
So, the empirical formula of the oxide is Ag2O.
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