Home
Class 12
CHEMISTRY
A current of 2.0A passed for 5 hours thr...

A current of 2.0A passed for 5 hours through a molten metal salt deposits 22.2 g of metal (At. Wt. =177). The oxidation state of the metal in the metal salt is

Text Solution

Verified by Experts

`Q="lt"=(2 amp)xx(5xx60xx60 s)=3600" C"`
Equivalent mass of metal
`=((22.2 g))/((36000C))xx(96500C)=59.5" g"`
Valency of metal`=("Atomic mass")/("Equivalent mass")=(177)/(59.5)=3`
Promotional Banner

Topper's Solved these Questions

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise COMPLETION QUESTION|2 Videos

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise NCERT In-Text Questions|9 Videos

  • ALDEHYDES AND KETONES

    DINESH PUBLICATION|Exercise Interger|5 Videos

Similar Questions

Explore conceptually related problems

The oxidation state of metal in metal carbonyl is

The oxidation stat of the metal in Reinecks salt is +x, x is

A current of 2.0 ampere is passed for 5.0 hour through a molten tin salt to deposit 22.2 g tin. What is the oxidation state of tin in salt? Atomic wt. of Sn = 118.69 g .

A current of 2A is passed for 1.93 xx 10^(4)s through a molten tin salt depositing 23.8 g Sn (Aw of Sn=119) . The oxidation state of Sn in the salt is ………………………… .

The oxidation number of the d-block metal in Zeises salt is