Question #76556
In a reaction it was found that 3.0g of a metal *X* was oxidized by 25.0 cm³ of 0.10 mol dm-³ K2 Cr2 O2 under acidic conditions.
(i) Deduce the mole of ratio between *X* and Cr2 O7²- ion.
(ii) write a balanced equation of the redox reaction.
(iii) Give the oxidation numbers of chromium and *X* in both their reduced and oxidized forms.
[Molar mass of *X* = 200.6]
(i) Deduce the mole of ratio between *X* and Cr2 O7²- ion.
(ii) write a balanced equation of the redox reaction.
(iii) Give the oxidation numbers of chromium and *X* in both their reduced and oxidized forms.
[Molar mass of *X* = 200.6]
Expert's answer
Learn more about our help with Assignments: Physical Chemistry
"assignmentexpert.com" is professional group of people in Math subjects! They did assignments in very high level of mathematical modelling in the best quality. Thanks a lot
#339914 on Dec 2023
#339914 on Dec 2023
Comments