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Metal deficiency defect is shown by \mathrm{Fe}_{0.93} \mathrm{O}. In the crystal, some \mathrm{Fe}^{2+} cations are missing and loss of positive charge is compensated by the presence of \mathrm{Fe}^{3+} ions. The percentage of \mathrm{Fe}^{2+}ions in the \mathrm{Fe}_{0.93} \mathrm{O} crystals is__________ . (Nearest integer)

Option: 1

85


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

\text { In } \text { Fe}_{0.93} \text{O}, Iron present as \text {Fe}^{+2} & \text {Fe}^{+3}

Suppose : \mathrm{\mathrm{Fe}^{2 +}=x, \mathrm{Fe}^{3 +}=0.93-x}

\mathrm{Fe_{0.93}O} is electrically neutral, thus charge balance on the compound gives us 

\begin{gathered} \mathrm{x \times 2+(0.93-x) \times 3-2 \times 1=0} \\ \mathrm{2 x+2.79-3 x-2=0} \\ \mathrm{x=.79} \end{gathered}

\mathrm{Fe}^{+2}=0.79, \mathrm{Fe}^{+3}=0.14

Percentage of \mathrm{Fe}^{2+} ion present

\begin{aligned} &=\frac{0.79}{0.93} \times 100=84.94 \% \\ &=85 \text { (Nearest integer) } \end{aligned}

Hence, answer is 85.

Posted by

jitender.kumar

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