Problem: 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.

FREE Expert Solution

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.

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Problem Details

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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What scientific concept do you need to know in order to solve this problem?

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