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The chloride of a metal contains 71% chl...

The chloride of a metal contains 71% chlorine by weight and the vapour density of it is 50. The atomic weight of the metal will be -

A

29

B

58

C

35.5

D

71

Text Solution

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The correct Answer is:
To find the atomic weight of the metal in the chloride, we can follow these steps: ### Step 1: Determine the Molecular Mass of the Chloride We know that the vapor density (VD) of the chloride is given as 50. The formula for vapor density is: \[ \text{Vapor Density} = \frac{\text{Molecular Mass}}{2} \] From this, we can rearrange the formula to find the molecular mass: \[ \text{Molecular Mass} = \text{Vapor Density} \times 2 \] Substituting the given vapor density: \[ \text{Molecular Mass} = 50 \times 2 = 100 \text{ g/mol} \] ### Step 2: Calculate the Weight of the Metal in the Chloride We know that the chloride contains 71% chlorine by weight. This means that in 100 g of the chloride, there are 71 g of chlorine. To find the weight of the metal in the chloride, we can subtract the weight of chlorine from the total weight of the chloride: \[ \text{Weight of Metal} = \text{Total Weight} - \text{Weight of Chlorine} \] \[ \text{Weight of Metal} = 100 \text{ g} - 71 \text{ g} = 29 \text{ g} \] ### Step 3: Determine the Atomic Weight of the Metal Since we have calculated that the weight of the metal in the chloride is 29 g, we can conclude that the atomic weight of the metal is: \[ \text{Atomic Weight of Metal} = 29 \text{ g/mol} \] ### Final Answer Thus, the atomic weight of the metal is **29 g/mol**. ---
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