# chemistry 101

posted by .

How many molecules of oxygen are produced from the decomposition of 8.75 g of hydrogen peroxide in the following equation Mg + H2O2 --> MgH2 + O2

options:

8.75 x 1024

6.02 x 1023

1.55 x 1022

5.27 x 1024

1.55 x 1023

• chemistry 101 -

Here is a worked example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html

• chemistry 101 -

8.75/34.02 (molar mass of H2O2) = .257 mol H2O2

Since the mol ratio b/t H2O2 and O2 is 1:1, there is also .257 mol O2

.257 mol * 6.02 * 10^23 = 1.55 * 10^24 molecules so the 3rd option.

## Similar Questions

1. ### Chemistry

The following reaction represents the decomposition of hydrogen peroxide: 2H2O2 -> O2 (g) + 2H2O (l) How many molecules of water are produced from the decomposition of 3.4g of hydrogen peroxide, H2O2?
2. ### Chemistry

The following reaction represents the decomposition of hydrogen peroxide 2H2O2 -> o2 (g) + 2H2O (l) How many molecules of water are produced from the decomposition of 3.4g of Hydrogen peroxide, H2O2?
3. ### Chemistry

Thank you for your help. I did want to clarify why you are only calculating the Molar Mass for H2 and not the molar mass for H2O (or even H2O2). I'm not sure why you did this. Please clarify. See below: The following reaction represents …
4. ### Chemistry

Oxygen gas and water are produced by the decomposition of hydrogen peroxide. If 10.0 mol of H2O2 decomposes, what volume of oxygen will be produced?
5. ### Chemistry - Mole Ratio

How many moles of oxygen are produced from the decomposition of 3.4g of hydrogen peroxide?
6. ### CHEMISTRY

The following reaction represents the decomposition of hydrogen peroxide: Balanced equation: 2H2O2 -> O2 + 2H2O How many moles of oxygen are produced from the decomposition of 3.4g of hydrogen peroxide?
7. ### chem

Oxygen gas and water are produced by the decomposition of hydrogen peroxide. If 10.0 mol of H2O2 decomposes, what volume of oxygen will be produced?
8. ### Chemistry

Oxygen gas may be prepared by decomposing hydrogen peroxide, h2o2, using manganese (IV) oxide catalyst: 2H2O2(liquid) ----> 2H2O(liquid) + O2(gas) Calculate the amount of oxygen that will be produced from 1.35 moles of H2O2 Determine …
9. ### science

Oxygen gas may be prepared by decomposing hydrogen peroxide, h2o2, using manganese (IV) oxide catalyst: 2H2O2(liquid) ----> 2H2O(liquid) + O2(gas) Calculate the amount of oxygen that will be produced from 1.35 moles of H2O2 Determine …
10. ### Chemistry

A student generated oxygen gas by decomposing hydrogen peroxide (H2O2) according to the following equation: 2H2O2(aq) -> 2H2O(l) + O2(g) If the student started with 1.75 moles of hydrogen peroxide, how many moles of oxygen gas would …

More Similar Questions