On reduction with hydrogen , 3.6 g of an...

On reduction with hydrogen , 3.6 g of an oxide of metal left 3.2 g of metal . If the simplest atomic weight of metal is 64, the simplest formula of the oxide is

A

MO

B

`M_2O_3`

C

`M_2O`

D

`M_2O_5`

Verified by Experts

The correct Answer is:

C

Similar Questions

Explore conceptually related problems

1.0 g of a metal oxide gave 0.2 g of metal. Calculate the equivalent weight of the metal.

5.6 g of a metal forms 12.7 g of metal chloride. Hence equivalent weight of the metal is

3 g of an oxide of a metal is converted completely to 5 g chloride. Equivalent weight of metal is:

3.0 g of metal chloride gave 2.0 g of metal. Calculate the equivalent weight of the metal.

A metal oxide contains 60% metal . The equivalent weight of metal is

An oxide of metal M has 40% by mass of oxygen. Metal M has relative atomic mass of 24. The empirical formula of the oxide is:

0.1 g of metal combines with 46.6 mL of oxygen at STP . The equivalent weight of metal is

70 gms of a metal oxide on reduction produced 54 gms of metal. The atomic weight of the metal is 81. What is its valency?

1.520 g of the hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent weight of metal is

74.5 g of a metallic chloride contain 35.5 g of chlorine. The equivalent weight of the metal is