Question

# A metal oxide (MO) is reduced by heating it in a stream of hydrogen. It is found that after complete reduction, 7.95 g of oxide requires 0.2gofH2 to yield 6.35 g of the metal. We may deduce that:

A
the atomic weight of the metal is 48.
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
the atomic weight of the metal is 16.
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
the atomic weight of the metal is 12.
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
the atomic weight of the metal is 63.5.
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution

## The correct option is D the atomic weight of the metal is 63.5.The balanced equation can be written as:MO+H2→M+H2O1 mole of MO requires = 1 mole of H2Now 0.2g of H2 = 0.1 mole of H2∴ For 0.1 mole of H2 = 0.1 mole of MO = 7.95g of MO is requiredIf 0.1mole of MO = 7.95g 1 mole of MO = 79.5gWeight of MO = M + 16 ∴ Atomic weight of metal(M) = 79.5 - 16 =63.5g

Suggest Corrections
0
Related Videos
Stoichiometric Calculations
CHEMISTRY
Watch in App