A) \[27.9~~~~~\]
B) \[159.6\]
C) \[79.8~\]
D) \[55.8\]
Correct Answer: D
Solution :
| The reaction may given as \[{{Z}_{2}}{{O}_{3}}+3{{H}_{2}}\xrightarrow{{}}2Z+3{{H}_{2}}O\] |
| \[0.1596g\]of \[{{\operatorname{Z}}_{2}}{{O}_{3}}\]react with \[{{\operatorname{H}}_{2}}=6\operatorname{mg}\]\[=0.006g\] |
| \[\therefore 1\,g\]of \[{{\operatorname{H}}_{2}}\]react with \[=\frac{0.1596}{0.006}=26.6\operatorname{g}\,of\,{{Z}_{2}}{{\operatorname{O}}_{3}}\] |
| \[\therefore \]Eq. wt. of \[{{Z}_{2}}{{O}_{3}}=26.6\] (from the definition of eq. wt.) |
| Eq. wt. of Z+ Eq. wt. of \[O=E+8=26.6\,\]\[\Rightarrow \]\[eq.wt.\,of\,Z=26.6-8=18.6\] |
| Valency of metal in \[{{Z}_{2}}{{O}_{3}}=3\] |
| Eq. wt. of metal \[=\frac{Atomic\,wt.}{valency}\] |
| \[\therefore \]At. Wt. of \[\operatorname{Z}=18.6\times 3=55.8\] |
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