4. FeCl_(3) weighs 5.95 g.The chloride converted to the hydrous oxide and ignited to Fe_(2)O_(3) The oxide weighs 2.62 g Calculate the percent Fe in the original mixture. chloride did the sample contain?

To calculate the percent Fe in the original mixture, we need to determine the mass of Fe in the original mixture and divide it by the total mass of the mixture.<br /><br />Given information:<br />- The mass of $FeCl_{3}$ is 5.95 g.<br />- The mass of the ignited oxide ($Fe_{2}O_{3}$) is 2.62 g.<br /><br />Step 1: Calculate the mass of Fe in the original mixture.<br />The mass of Fe in the original mixture can be calculated by subtracting the mass of the ignited oxide ($Fe_{2}O_{3}$) from the mass of $FeCl_{3}$.<br /><br />Mass of Fe = Mass of $FeCl_{3}$ - Mass of $Fe_{2}O_{3}$<br />Mass of Fe = 5.95 g - 2.62 g = 3.33 g<br /><br />Step 2: Calculate the percent Fe in the original mixture.<br />Percent Fe = (Mass of Fe / Total mass of the mixture) × 100<br />Percent Fe = (3.33 g / 5.95 g) × 100 = 55.8%<br /><br />Therefore, the percent Fe in the original mixture is 55.8%.