what is the balanced net ionic equation for the oxidation of hydrogen peroxide by permanganate ion and find out how many moles of hydrogen peroxide react with one mole of permanganate ion.
would the answer be:
2MnO4^- + 6h^+ + 5H2O2 ---> 2Mn^2+ + 8H2O + 5O2
ratio of 2:5
0.4 moles ?
sorry, H2O2:MnO4 = 5:2, not 2:5
yeah, that's what i meant..
but is the number of moles correct?
no, you'd need 1/.4 = 2.5 moles.
Since 5 moles react with 2, 2.5 moles react with 1.
Yes, you're correct. The balanced net ionic equation for the oxidation of hydrogen peroxide (H2O2) by permanganate ion (MnO4-) is:
2MnO4^- + 6H^+ + 5H2O2 --> 2Mn^2+ + 8H2O + 5O2
In this equation, two moles of permanganate ion and five moles of hydrogen peroxide react to form two moles of manganese (II) ion, eight moles of water, and five moles of oxygen gas. So, the ratio of hydrogen peroxide to permanganate ion is 5:2.
To find out how many moles of hydrogen peroxide react with one mole of permanganate ion, you can use the ratio from the balanced equation:
5 moles H2O2 : 2 moles MnO4^-
So, for one mole of MnO4^-, you would need (5/2) moles of H2O2, which is equal to 2.5 moles of H2O2.
Therefore, one mole of permanganate ion reacts with 2.5 moles of hydrogen peroxide.