5.0g of an oxide of a metal n gave 4.0g of the metal when reduced with hydrogen what is the empirical formula of the oxide.
To determine the empirical formula of the oxide, we need to analyze the given information and calculate the molar ratios between the metal and oxygen.
First, we need to find the number of moles of both the metal and the oxygen in the given amounts.
1. Calculate the number of moles of the metal (n) using its given mass:
Moles of Metal (n) = Mass of Metal (given) / Molar Mass of Metal
2. Calculate the number of moles of oxygen:
Moles of Oxygen = Moles of Metal (n) - Moles of Metal (obtained during reduction)
3. Determine the ratios of the moles of metal to oxygen and simplify them to whole numbers:
Divide both the moles of metal and moles of oxygen by the smallest of the two values. If both values are already whole numbers, proceed to step 4.
4. Use the simplified whole-number ratios to determine the empirical formula of the oxide:
Write the empirical formula with the metal symbol followed by the subscript of its moles, then the oxygen symbol followed by the subscript of its moles.
Let's calculate the empirical formula step by step using the given information:
Given:
Mass of Metal (n) = 4.0g
Mass of Oxide (nO) = 5.0g
1. Calculate the number of moles of metal (n):
Molar Mass of Metal (M) = ? (not given)
We will assume the molar mass of n is 1g/mol for simplicity.
Moles of Metal (n) = Mass of Metal (given) / Molar Mass of Metal
Moles of Metal (n) = 4.0g / 1g/mol
Moles of Metal (n) = 4.0 mol
2. Calculate the number of moles of oxygen (O):
Moles of Oxygen (O) = Moles of Metal (n) - Moles of Metal (obtained during reduction)
Moles of Oxygen (O) = 4.0 mol - 4.0 mol (since all of the metal is obtained during reduction)
Moles of Oxygen (O) = 0 mol
3. Determine the ratios of the moles of metal (n) to oxygen (O) and simplify:
Since there are no moles of oxygen (O) present, the ratio is 4.0:0 or simply 4:0.
4. Write the empirical formula of the oxide:
The empirical formula is written with the metal symbol (n) followed by the subscript of its moles (4) and without writing the oxygen symbol since there are no moles of oxygen in this case.
Therefore, the empirical formula of the oxide is n4.
Note: The empirical formula obtained is based on the given information and assumptions made for the molar mass of n. If the actual molar mass of n is known, the calculations should be adjusted accordingly.