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3 years ago

Select the correct answer.

Chemistry

1 answer:

muminat3 years ago

7 0

Answer:- B. 4.65 g.

Solution:- The given balanced equation is:

$2AgNO_3(aq)+Na_2S(aq)\rightarrow Ag_2S(s)+2NaNO_3(aq)$

It asks to calculate the mass of silver sulfide formed by when 0.0150 liters of 2.50 M of silver nitrate are used.

Moles of silver nitrate are calculated on multiplying it's liters by its molarity and then on multiplying by mol ratio, the moles of silver sulfide are calculated. These moles are multiplied by the molar mass to convert to the grams.

Molar mass of $Ag_2S$ = 2(107.87)+32.06 = 247.8 g per mol

The dimensional set up for the complete problem is:

$0.0150L(\frac{2.50molAgNO_3}{1L})(\frac{1molAg_2S}{2molAgNO_3})(\frac{247.8gAg_2S}{1molAg_2S})$

= $4.65gAg_2S$

So, the correct choice is B. 4.65 g.

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First we need to calculate the number of moles of FeS $_{2}$ :

number of moles = mass (grams) / molecular mass (g/mol)

number of moles of FeS $_{2}$ = 198.2/120 = 1.65 moles

From the chemical reaction we deduce that:

if 4 moles of FeS $_{2}$ produces 8 moles of SO $_{2}$

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