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12 Nov 2019
A piece of iron weighting 85.65 g was burned in air. The mass of the irons oxide produced was 118.37g. Use the molar mass of iron to covert the mass of iron used to moles. According to the law of conservation of mass, what is the mass of oxygen that reduced with the iron? Calculate the number of moles of oxygen in the product. Use the ratio between the number of moles of iron and number of moles of oxygen to calculate the empirical formula of iron oxide. Note: Fractions of atoms do not exist in compounds. In the case where the ratio of atoms is a fractional number, such as 1/2, the ratio should be simplified by multiplying all the atoms by a constant to give whole number rations for all atoms (e. g. , Ho1/2 should be H2O). Silver oxide samples oxides samples, 0.5g Balance, milligram(0.001 - g precision) Crucible and crucible lid, 15 - or 30 ml. Clay pipe stem triangle Crucible tongs Wire gauze with ceramic center
A piece of iron weighting 85.65 g was burned in air. The mass of the irons oxide produced was 118.37g. Use the molar mass of iron to covert the mass of iron used to moles. According to the law of conservation of mass, what is the mass of oxygen that reduced with the iron? Calculate the number of moles of oxygen in the product. Use the ratio between the number of moles of iron and number of moles of oxygen to calculate the empirical formula of iron oxide. Note: Fractions of atoms do not exist in compounds. In the case where the ratio of atoms is a fractional number, such as 1/2, the ratio should be simplified by multiplying all the atoms by a constant to give whole number rations for all atoms (e. g. , Ho1/2 should be H2O). Silver oxide samples oxides samples, 0.5g Balance, milligram(0.001 - g precision) Crucible and crucible lid, 15 - or 30 ml. Clay pipe stem triangle Crucible tongs Wire gauze with ceramic center
Bunny GreenfelderLv2
11 May 2019