Hydrogen peroxide, H2O2, is unstable under certain conditions and decomposes as follows:
2 H2O2 → 2 H2O + O2
? g 34.00 g 15.98 g
What mass of hydrogen peroxide, to the nearest hundredth of a gram, is decomposed in this reaction?
Please help 😔
That question is flawed or there is a typo somewhere. 49.98 SHOULD BE the correct answer BUT if you start with 49.98 g H2O2 and decompose all of it you do NOT get 34.00 g H2O and 15.98 g O2. Starting with 49.98 g H2O2 will give you 26.46 g H2O and 23.52 g O2.
Mrs. Sue died due to sickness. I came here looking for the answer too. The best answer I have is 49.98. I added 15.98g and 34g. I'm not sure if it's right but it's the best I got.
RIP Mrs. Sue. Fly High. Thank you for all the help.
I do need help :')
To find the mass of hydrogen peroxide decomposed in this reaction, we need to use the molar masses of hydrogen peroxide and oxygen.
The molar mass of hydrogen peroxide (H2O2) is calculated by summing the atomic masses of its components:
H2O2:
2 hydrogen (H) atoms: 2 * 1.008 g/mol = 2.016 g/mol
2 oxygen (O) atoms: 2 * 16.00 g/mol = 32.00 g/mol
Total molar mass = 2.016 g/mol + 32.00 g/mol = 34.016 g/mol (approximately 34.02 g/mol)
From the balanced chemical equation, we see that two moles of hydrogen peroxide decompose to form two moles of water (H2O) and one mole of oxygen (O2).
So, the molar ratio of H2O2 to O2 is 2:1.
Given that 34.00 g of H2O is formed per mole of H2O2, we can calculate the mass of H2O2 decomposed:
34.00 g H2O2 * (1 mole H2O2 / 34.02 g H2O2) = 1.00 mole H2O2
Since the molar ratio of H2O2 to O2 is 2:1, we can calculate the moles of O2 formed:
1.00 mole H2O2 * (1 mole O2 / 2 moles H2O2) = 0.50 moles O2
Finally, we can find the mass of O2 formed:
0.50 moles O2 * (32.00 g O2 / 1 mole O2) = 16.00 g O2
Therefore, approximately 16.00 grams of hydrogen peroxide are decomposed in this reaction.