Pre-Lab Questions A piece of iron weighing 85.65 g was burned in air. The mass of the iron oxide produced was 118.37 g. 1. Use the law of conservation of mass to calculate the mass of oxygen that reacted with the iron. 2. Use the molar mass of oxygen to calculate the number of moles of oxygen atoms in the product. 3. Use the molar mass of the iron to convert the mass of iron used to moles. 4. Use the ratio between the number of moles of iron and the number of moles of oxygen atoms to calculate the empirical formula of iron oxide. Note: Fractions of ato ms do not exist. In the case where the ratio of atoms results in a decimal fraction, such as 1.5:1, the ratio should be simplified by converting it to the nearest whole number ratio. For example, the ratio 1.5:1 is multiplied by two to convert to a whole number ratio of 3:2.

Pre-Lab Questions A piece of iron weighing 85.65 g was burned in air. The mass of the iron oxide produced was 118.37 g. 1. Use the law of conservation of mass to calculate the mass of oxygen that reacted with the iron. 2. Use the molar mass of oxygen to calculate the number of moles of oxygen atoms in the product. 3. Use the molar mass of the iron to convert the mass of iron used to moles. 4. Use the ratio between the number of moles of iron and the number of moles of oxygen atoms to calculate the empirical formula of iron oxide. Note: Fractions of ato ms do not exist. In the case where the ratio of atoms results in a decimal fraction, such as 1.5:1, the ratio should be simplified by converting it to the nearest whole number ratio. For example, the ratio 1.5:1 is multiplied by two to convert to a whole number ratio of 3:2.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 10QAP: Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion,...

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A piece of iron weighing 85.65 g was burned in air. The mass of the iron oxide produced was 118.37 g.1. Use the law of conservation of mass to calculate the mass of oxygen that reacted with the iron.2. Use the molar mass of oxygen to calculate the number of moles of oxygen atoms in the product.3. Use the molar mass of the iron to convert the mass of iron used to moles.4. Use the ratio between the number of moles of iron and the number of moles of oxygen atoms to calculate the empirical formula of iron oxide. JUST Need HELP ON NUMBER 3 AND 4
A piece of iron weighing 85.65 g was burned in air. The mass of the iron oxide produced was 118.37 g.1. Use the law of conservation of mass to calculate the mass of oxygen that reacted with the iron.2. Use the molar mass of oxygen to calculate the number of moles of oxygen atoms in the product.3. Use the molar mass of the iron to convert the mass of iron used to moles.4. Use the ratio between the number of moles of iron and the number of moles of oxygen atoms to calculate the empirical formula of iron oxide.
Im supposed to find the molar ratio and the empiricle formula from my data but im confused. At the bottom left is where I'm trying to find the moles of each substance. Am I doing this right? help.