One gram of a metallic chloride was found to contain $0.835 g$ of chlorine. Its vapour density metallic chloride is $85.5$ . If its molecular formula is $M_{x} C l_{y}$ , then what is the value of $(x + y)$ ?

Open in App

Solution

x=1 and y= 4
so x+y =5

Suggest Corrections

Similar questions

(a) A metal M forms a volatile chloride containing 65.5% chlorine. If the density of the chloride relative to hydrogen is 162.5, find the molecular formula of the chloride.
(M = 56; Cl = 35.5)

Q. A metal Z forms a volatile chloride containing 65.5% chlorine. If the density of the chloride relative to hydrogen is 162.5,find the molecular formula of the metal chloride(Z=56, Cl=35.5)

Q. A transition metal

M

forms a volatile chloride which has a vapour density of

94.8

. If it contains

74.75

% of chlorine the formula of the metal chloride will be:

Q. The chloride of a metal contains 71% of chlorine by weight and its vapour density is 50.What will be the atomic weight of the metal?

Q. The chloride of a metal contains 71% of chlorine by mass and its vapour density is 50. The atomic mass of metal will be??

Join BYJU'S Learning Program

One gram of a metallic chloride was found to contain 0.835g of chlorine. Its vapour density metallic chloride is 85.5. If its molecular formula is MxCly, then what is the value of (x+y) ?

x=1 and y= 4so x+y =5

One gram of a metallic chloride was found to contain $0.835 g$ of chlorine. Its vapour density metallic chloride is $85.5$ . If its molecular formula is $M_{x} C l_{y}$ , then what is the value of $(x + y)$ ?

x=1 and y= 4
so x+y =5