In a titration experiment, H2O2(aq) reacts with aqueous MnO4-(aq) as represented by the equation above. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. (Note: At the end point of the titration, the solution is a pale pink color.)
At a certain time during the titration, the rate of appearance of O2(g) was 1.0 x 10-3 mol/(L⋅s). What was the rate of disappearance of MnO4- at the same time. (please explain it)
Options
6.0 x 10-3 mol/(L⋅s)
A
4.0 x 10-3 mol/(L⋅s)
B
6.0 x 10-4 mol/(L⋅s)
C
4.0 x 10-4 mol/(L⋅s)
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Ответ:
C. 4x10⁻⁴ mol / (Ls)
Explanation:
Based in the reaction:
5 H₂O₂(aq) + 2 MnO₄⁻(aq) + 6 H⁺(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 O₂(g)
2 moles of MnO₄⁻ disappears while 5 moles of O₂ appears.
If 5 moles appears in a rate of 1.0x10⁻³mol /(Ls), 2 moles will disappear:
2 moles ₓ (1.0x10⁻³mol /(Ls) / 5 moles) = 4x10⁻⁴ mol / (Ls)
Right answer is:
C. 4x10⁻⁴ mol / (Ls)
Ответ:
A decrease in injuries and death (APEX)