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 maximum mass (in gm) of precipitate any of beaker ?

Answer:

71.75

Solution:

(1) $2 AgNa_{3} + CaCl_{2} * \to 2 AgCl (s) \to 0.30$ mole $AgCl (s)$ (Minimum) $\Rightarrow 43.05 gm$ 0.5 mole 0.15 mole

(2) $3 * AgNO_{3} + AlCl_{3} ⟶ 3 AgCl (s) \to 0.5$ mole $AgCl (s)$ (Maximum $\Rightarrow 71.75 gm$

0.5 mole 0.20 mole

(3) $2 AgNO_{3} + CaCl_{2} \to 2 AgCl (s) \to 0.5$ mole $AgCl (s)$

0.5 mole 0.25 mole

(4) $AgNO_{3} + NaCl * ⟶ AgCl (s) ⟶ 0.30$ mole $AgCl (s)$

$0.5$ mole $0.30$ mole

(5) $AgNO_{3} + NaCl * ⟶ AgCl (s) ⟶ 0.40$ mole $AgCl (s)$

$0.5$ mole $0.40$ mole

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

⏱ 2mℹ️ Source: QB

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