Question
A certain metal oxide has the formula $\mathrm{MO},$ where $\mathrm{M}$ denotes the metal. A $39.46-\mathrm{g}$ sample of the compound is strongly heated in an atmosphere of hydrogen to remove oxygen as water molecules. At the end, $31.70 \mathrm{~g}$ of the metal is left over. If $\mathrm{O}$ has an atomic mass of 16.00 amu, calculate the atomic mass of $\mathrm{M}$ and identify the element.
Step 1
The initial mass of the compound is 39.46 g, and the mass of the metal left after heating is 31.70 g. Therefore, the mass of oxygen removed is: \[ \text{Mass of oxygen} = 39.46 \, \text{g} - 31.70 \, \text{g} = 7.76 \, \text{g} \] Show more…
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A certain metal oxide has the formula MO where $M$ denotes the metal. A 39.46-g sample of the compound is strongly heated in an atmosphere of hydrogen to remove oxygen as water molecules. At the end, 31.70 g of the metal is left over. If O has an atomic mass of 16.00 amu, calculate the atomic mass of $\mathrm{M}$ and identify the element.
A certain metal oxide has the formula MO where M denotes the metal. A 39.46-g sample of the compound is strongly heated in an atmosphere of hydrogen to remove oxygen as water molecules. At the end, $31.70 \mathrm{g}$ of the metal is left over. If $\mathrm{O}$ has an atomic mass of 16.00 amu, calculate the atomic mass of $M$ and identify the element.
DETERMINATION OF ATOMIC MASS A 1.443-gram sample of metal is reacted with excess oxygen to yield $1.683$ grams of the oxide $\mathrm{M}_{2} \mathrm{O}_{3}(s) .$ Calculate the atomic mass of the element $\mathrm{M}$ and identify the metal.
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