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Chemistry - Stoichiometry Question with Solution | TestHub

ChemistryStoichiometryBasic Methods of Calculations (POAC, LR)Medium2 minQB

ChemistryMediumnumerical

Passage / Comprehension

Five beakers (labelled 1 to 5) each contain 0.5 moles of silver nitrate ( $AgNO_{3}$ ) dissolved in water. Into each of these beakers is added a certain amount of a metal chloride, as shown in the table below. Silver chloride precipitates from the solution in all five beakers.

(Given: Molar mass of $AgCl$ is 143.5 gm/mole).

What is minimum mass (in gm ) of precipitate in any of beaker ?

Answer:

43.05

Solution:

Moles of $Ag^{+} = 0.5$

Minimum mass will be formed by solution having minimum $Cl^{-}$ which is 0.3 mole.

So moles of AgCl formed $= 0.3$

So mass of AgCl formed $= 0.3 \times 143.5$

$= 43.05$

Stream:JEESubject:ChemistryTopic:StoichiometrySubtopic:Basic Methods of Calculations (POAC, LR)

⏱ 2mℹ️ Source: QB

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