32.1 g of a metal were dissolved in HCl and the hydrogen evolved was burnt to form water which weighed  9.1 g. The specific heat of the metal is   0.094. Calculate its at. wt.

(i) Wt. of metal =32.1g;wt. of H2O=9.1g. 18 g H2O contains H2        =2g                  ∵H2O≡2H;18= mol. wt. of H2O∴9.1gH2O contains  H2=218×9.1=1.01g we know , Wt. of metal  Wt. of H2= Eq. wt. of metal  Eq. wt. of H2(=1);32.11.01=E1∴ E=31.78 (ii) Approx. at. wt. =6.4 sp. heat =6.40.094=68.08 ∴  Valency = Approx. at. wt.  Eq. wt. =68.0831.78                =2.1≈2  Exact at. wt. = Eq. wt. × Valency =31.78×2=63.56