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frutty [35]
3 years ago
12

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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Answer:

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<em>Refer to the equation in BaSO₄ as an example. Try setting up the equation on your own. </em>

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Ions carry charge. Oxidation states on atoms in an ion shall add up to the charge of the ion. The superscript of an ion shows its charge. The superscript 3- in the phosphate ion shows that the ion carries a charge of -3.

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