Q: When vanadium reacts with chlorine at 400°C, a brown compound is obtained. When an
aqueous solution containing 0.193 g of this compound was treated with aqueous silver nitrate all the chlorine in the compound was precipitated as silver chloride. The mass of silver chloride (AgCl) produced was 0.574 g. Which one of the following could be the formula of the brown compound?
A VCl
B VCl2
C VCl3
D VCl4
I'm not exactly sure what to do here?
I've tried to work out the total mass of chlorine that is present in silver chloride as I think that might be important here.
So this gave me '0.142 g' by doing '35.5/143.5' which is known to be fraction of how much chlorine makes up the silver chloride compound and then multiplying it by the total mass of silver chloride '0.574 g' giving '0.142 g' of chlorine that exists in the silver chloride
What would the next step be now? Do I need to somehow maybe set up an equation of vanadium reacting with AgCl that will help give a molar ratio or something?
I'm not too sure.
Any help would be nice. Thanks a lot!