We’re being asked to determine the empirical formula of the second compound formed when a mass of element X is combined with different mass of element Z.
Recall that the empirical formula is the lowest whole number ratio of elements present in a compound.
The second compound is formed when 1.00 g of element X is combined with 0.315 g of element Z. The first compound is formed when 1.00 g of element X is combined with 0.472 g of element Z and has a formula of X2Z3
We will do the following steps to solve the problem:
Step 1: Determine the ratio in mass of each element in the first compound
Step 2: Determine the lowest whole number mole ratio of the second compound to get the empirical formula.
Three pure compounds are formed when 1.00-g samples of element X combine with, respectively, 0.472 g, 0.315 g , and 0.944 g of element Z. The first compound has the formula X2 Z3.
Find the empirical formula of the second compound.
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