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.

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

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:

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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?

Our tutors have indicated that to solve this problem you will need to apply the Atomic Theory concept. You can view video lessons to learn Atomic Theory. Or if you need more Atomic Theory practice, you can also practice Atomic Theory practice problems.

What professor is this problem relevant for?

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