The atomic weight of element X is 100 g/mol. 50 grams of X combines with 32.0 g of oxygen. What is the simplest formula for the resulting compound?

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The atomic weight of element X is 100 g/mol. 50 grams of X combines with 32.0 g of oxygen. What is the simplest formula for the resulting compound?

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Answer 1 · 2014-10-08T01:48:52

The simplest formula of the compound is XO₄.

Step 1. Determine the moles of each element

Moles of X = 50 g X × $\frac{1 mol X}{100 g X}$ $"1 mol X"/"100 g X"$ = 0.50 mol X

Moles of O = 32.0 g O × $\frac{1 mol O}{16.00 g O}$ $"1 mol O"/"16.00 g O"$ = 2.00 mol O

Step 2. Determine the Molar Ratios

$\frac{Moles of X}{Moles of O} = \frac{0.50 mol}{2.00 mol} = \frac{1}{4.0} \approx \frac{1}{4}$ $"Moles of X"/"Moles of O" = "0.50 mol"/"2.00 mol" = 1/4.0 ≈ 1/4$

Step 3. Write the Simplest Formula

The empirical formula of the oxide is XO₄.

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The atomic weight of element X is 100 g/mol. 50 grams of X combines with 32.0 g of oxygen. What is the simplest formula for the resulting compound?

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