What is the molar mass of the compound represented by the following structural formula?
- A$36 \ g \ mol^{-1}$
- B$46 \ g \ mol^{-1}$
- C$22 \ g \ mol^{-1}$
- D$32 \ g \ mol^{-1}$
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Similar Questions
$71 \ g$ of chlorine combines with a metal to form $111 \ g$ of its chloride. The chloride is isomorphous with $MgCl_2 \cdot 6H_2O$. The atomic weight of the metal is:
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View SolutionCalculate the average atomic mass of chlorine using the following data:
Isotope Natural abundance (%) Molar mass $(u)$ $^{35}Cl$ $75.77$ $34.9689$ $^{37}Cl$ $24.23$ $36.9659$
(in $u$)
| Isotope | Natural abundance (%) | Molar mass $(u)$ |
|---|---|---|
| $^{35}Cl$ | $75.77$ | $34.9689$ |
| $^{37}Cl$ | $24.23$ | $36.9659$ |
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View SolutionUpon fully dissolving $2.0 \ g$ of a metal in sulphuric acid,$6.8 \ g$ of the metal sulphate is formed. The equivalent weight of the metal is $...... \ g$.
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View SolutionThe equivalent mass of iodine in the following reaction is $I_2 + 2S_2O_3^{2-} \longrightarrow 2I^{-} + S_4O_6^{2-}$
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View Solution$1 \ g$ of a metal nitrate produces $0.86 \ g$ of metal sulphate. The equivalent weight of the metal will be:
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