Redox and Equivalent ConceptHard

Question

A quantity of 1.878 g of a metal bromide when heated in a stream of hydrogen chloride gas is completely converted to the chloride weighing 1.00 g. The specific heat of the metal is 0.14 cal/oc-g. What is the molecular weight of the bromide? (Br = 80, Cl = 35.5)

Options

A.45.54
B.125.54
C.285.54
D.205.54

Solution

neq metal bromide = neq metal chloride

Or $\frac{1.878}{E + 80} = \frac{1.00}{E + 35.5} \Rightarrow$Equivalent mass of metal, E = 15.18

Now, approximate atomic mass of metal = $\frac{6.4}{0.14}$ = 45.71

Valency = $\frac{45.71}{15.18}$ = 3 (integer)

Exact atomic mass of metal bromide = $15.18 \times 3$= 45.54

Molecular mass of metal bromide = $45.54 + 3 \times 80$= 285.54

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