Question 1
A sample of iron is heated in excess oxygen. The mass of iron used is 2.80 g and the mass of the iron oxide produced is 4.00 g. Determine the empirical formula of the iron oxide formed.
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Chemistry · Unit 1 · Chemical reactions — reactants, products and energy change · Chemical reactions
the empirical formula of a compound from reactions involving mass change
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Question 2
A student heated a sample of iron powder in air and measured the mass change. The iron powder had an initial mass of 5.60 g. After heating to constant mass, the product weighed 8.00 g. Determine the empirical formula of the iron oxide formed.
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