# Problem: Hydrogen and oxygen form both water and hydrogen peroxide. A decomposition of a sample of water forms 0.125 g hydrogen to every 1.00 g oxygen. The decomposition of a sample of hydrogen peroxide forms 0.0625 g hydrogen to every 1.00 g oxygen.Show that these results are consistent with the law of multiple proportions.

###### FREE Expert Solution
• Law of Multiple Proportions states that "When two elements form a series of compounds, the ratio of the masses of the 1st element that combine with 1 g of the other element can always be reduced to small whole numbers"

• In order to confirm the Law of Multiple Proportions here, we need to  calculate the mass of H over mass of O to find how much g of H is in 1 g of O

• Hydrogen peroxide is composed of a peroxide ion (O22-) and 2 H+ atoms. Recall that compounds, the charge of the ion goes to the subscript of the counterion. Hydrogen peroxide will appear as H2O2

• Calculating the proportions of H and O for water and hydrogen peroxide:

96% (190 ratings) ###### Problem Details

Hydrogen and oxygen form both water and hydrogen peroxide. A decomposition of a sample of water forms 0.125 g hydrogen to every 1.00 g oxygen. The decomposition of a sample of hydrogen peroxide forms 0.0625 g hydrogen to every 1.00 g oxygen.

Show that these results are consistent with the law of multiple proportions.

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

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Based on our data, we think this problem is relevant for Professor Brewer's class at UARK.