A) 8.2%
B) 25%
C) 16%
D) unpredictable
Correct Answer: A
Solution :
Molecular formula of ferrous fumarate is\[H{{e}^{+}}=\frac{1}{\lambda }={{R}_{H}}.{{Z}^{2}}\left[ \frac{1}{n_{2}^{2}}-\frac{1}{n_{2}^{2}} \right]\], molar mass is 170 \[={{R}_{H}}{{(2)}^{2}}\left[ \frac{1}{{{2}^{2}}}-\frac{1}{{{4}^{2}}} \right]\] 100 mg of\[=4{{R}_{H}}\times \frac{3}{16}=\frac{3}{4}{{R}_{H}}\]contains\[\text{s }>\text{ p}>\text{ d}>\text{ f}\]\[CsCl\] Total Fe in 400 mg of capsule\[C{{l}^{-}}\] \[\text{C}{{\text{s}}^{+}}\] percentage of Fe in capsule\[\frac{1}{8}\times 8=1\]
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