\( \mathrm{NX} \) is produced by the following step of reactions: \[ \begin{array}{l} \mathrm{M}...
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0\( \mathrm{NX} \) is produced by the following step of reactions:
\[
\begin{array}{l}
\mathrm{M}+\mathrm{X}_{2} \rightarrow \mathrm{MX}_{2}, 3 \mathrm{MX}_{2}+\mathrm{X}_{2} \rightarrow \mathrm{M}_{3} \mathrm{X}_{8}, \mathrm{M}_{3} \mathrm{X}_{8}+\mathrm{N}_{2} \mathrm{CO}_{3} \rightarrow \\
\mathrm{NX}+\mathrm{CO}_{2}+\mathrm{M}_{3} \mathrm{O}_{4}
\end{array}
\]
How much \( \mathrm{M} \) (metal) is consumed to produce \( 206 \mathrm{~g} \) of \( \mathrm{NX} \).
(Take at wt. of \( \mathrm{M}=56, \mathrm{~N}=23, \mathrm{X}=80 \) )
(a) \( 42 \mathrm{~g} \)
(b) \( 56 \mathrm{~g} \)
(c) \( \frac{14}{3} \)
(d) \( \frac{7}{4} \)
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