A) 14%
B) 15.05%
C) 17%
D) 29%
Correct Answer: B
Solution :
[b] \[F{{e}_{0.93}}{{O}_{1.00}}\] |
Oxidation number of \[F{{e}_{0.93}}\] |
= + 2 (0.93 mol possess net + 2 charge) |
Suppose x mol + 2 charge. |
then 0.93 - x posses + 3 charge |
Hence, \[x\times 2+3(0.93-x)=+2\] |
\[x=0.79\,F{{e}^{2+}};\,F{{e}^{3+}}=0.14\] |
\[F{{e}^{3+}}%=\frac{0.14}{0.93}\times 100=15.05%\] |
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