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Chapter 4: Problem 49

Consider the reaction below: \(2 \mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq}) \longrightarrow\) $$ \mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})+2 \mathrm{NaNO}_{3}(\mathrm{aq}) $$ (a) How many grams of \(\mathrm{Na}_{2} \mathrm{S}(\mathrm{s})\) are required to react completely with \(27.8 \mathrm{mL}\) of \(0.163 \mathrm{M} \mathrm{AgNO}_{3} ?\) (b) How many grams of \(\mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})\) are obtained from the reaction in part (a)?

Short Answer

Expert verified
(a) The mass of Na2S required to react completely is 0.1766 grams. (b) The mass of Ag2S obtained from the reaction is 0.5604 grams.

Step by step solution

01

Calculation of Moles of AgNO3

The moles of AgNO3 can be calculated using the formula:Moles = Molarity (M) × Volume (L)Given Molarity = 0.163M and Volume = 27.8 mL = 0.0278 LMoles = 0.163 × 0.0278 = 0.004526 moles
02

Find the Moles of Na2S

From the balanced chemical equation, the stoichiometric ratio of AgNO3 to Na2S is 2:1. Thus, the number of moles of Na2S that will react with AgNO3 is: Moles of Na2S = Moles of AgNO3 / 2 = 0.004526 /2 = 0.002263 moles
03

Find the Mass of Na2S Required

The molar mass of Na2S (sodium sulfide) is 78.045 g/mol. The mass of sodium sulfide (Na2S) can be calculated using the following formula:Mass (g) = Moles × Molar mass Mass (g) = 0.002263 moles × 78.045 g/mole = 0.1766 grams
04

Find the moles of Ag2S Produced

From the balanced chemical equation, the stoichiometric ratio of AgNO3 to Ag2S is 2:1. Thus, the number of moles of Ag2S produced is : Moles of Ag2S = Moles of AgNO3 / 2 = 0.004526 /2 = 0.002263 moles
05

Find the Mass of Ag2S Produced

The molar mass of Ag2S (silver sulfide) is 247.8 g/mol.The mass (g) of silver sulfide (Ag2S) can be calculated using the same formula as indicated previously: Mass (g) = Moles × Molar mass Mass (g) = 0.002263 moles × 247.8 g/mole = 0.5604 grams

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Most popular questions from this chapter

Titanium tetrachloride, \(\mathrm{TiCl}_{4}\) is prepared by the reaction below. $$\begin{aligned} &3 \mathrm{TiO}_{2}(\mathrm{s})+4 \mathrm{C}(\mathrm{s})+6 \mathrm{Cl}_{2}(\mathrm{g}) \longrightarrow 3 \mathrm{TiCl}_{4}(\mathrm{g})+2 \mathrm{CO}_{2}(\mathrm{g})+2 \mathrm{CO}(\mathrm{g}) \end{aligned}$$ What is the maximum mass of \(\mathrm{TiCl}_{4}\) that can be obtained from \(35 \mathrm{g} \mathrm{TiO}_{2^{\prime}} 45 \mathrm{g} \mathrm{Cl}_{2^{\prime}}\) and \(11 \mathrm{g} \mathrm{C} ?\)

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