Suppose that you could decompose 0.250 mol of Ag2S into its elements. a. How many moles of silver would you have? How many moles of sulfur would you have? b. How many moles of Ag2S are there in 38.8 g of Ag2S? How many moles of silver and sulfur would be produced from this amount of Ag2S? c. Calculate the masses of silver and sulfur produced in (b).
Answers
Answer:
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Explanation:
refer attachment
Answer:
The final answer is:
a) Number of moles of silver = 0.5 moles
Number of moles of sulfur = 0.25 moles
b) Number of moles of Ag₂S = 0.156 moles
Number of moles of silver = 0.313 moles
Number of moles of sulfur = 0.156 moles
c) Mass of silver produced in (b) = 33.77 grams
Mass of sulfur produced in (b) = 5.001 grams
Explanation:
Given that,
0.25 mol of Ag₂S is decomposed into its elements. So the decomposition is :
Ag₂S ---> 2 Ag + S
a) According to the above reaction,
1 mole of Ag₂S yields 2 moles of Ag (silver)
So, 0.25 moles of Ag₂S yields = 0.25 × 2 moles of Ag = 0.5 moles of Ag.
Similarly, 1 mole of Ag₂S yields 1 mole of S (sulfur)
So, 0.25 moles of Ag₂S yields = 0.25 × 1 moles of S = 0.25 moles of S.
b) Given that,
Number of grams of Ag₂S = 38.8 grams
Molecular mass of Ag₂S= 2 × Molecular mass of Ag +Molecular mass of S
= 2 × 107.86 + 32.06
= 247.80
Number of moles of Ag₂S = Number of grams of Ag₂S / Molecular mass of Ag₂S
= 38.8 / 247.80
= 0.156 moles
1 mole of Ag₂S yields 2 moles of Ag (silver)
So, 0.156 moles of Ag₂S yields=0.156 × 2 = 0.313 moles of Ag.
Similarly, 1 mole of Ag₂S yields 1 mole of S (sulfur)
So, 0.156 moles of Ag₂S yields = 0.156 × 1 moles of S = 0.156 moles of S.
c) Mass of Ag (silver) produced = Number of moles of Ag × Molecular mass of Ag
= 0.313 × 107.86
= 33.77 grams
Mass of S (sulfur) produced = Number of moles of S × Molecular mass of S
= 0.156 × 32.06
= 5.001 grams
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