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The tarnish that forms on objects made of silver is solid silver sulfide; it can be removed by reacting it with aluminum metal to produce silver metal and solid aluminum sulfide. How many moles of the excess reactant remain unreacted when the reaction is over if 5 moles of silver sulfide react with 8 moles of aluminum metal? Hint: Write a balanced chemical equation first. Enter to 1 decimal place.

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princessesther2011

Answer:

4.7 moles

Explanation:

Equation of reaction:

3Ag2S + 2Al = 6Ag +Al2S3

From the equation of reaction above,

3 moles of silver sulfide reacted with 2 moles of aluminum metal

Therefore, 5 moles of silver sulfide is required to react with (5×2/3 = 3.3 moles) of aluminum metal

The excess reactant is aluminum metal

Number of moles of aluminum metal that remain unreacted = 8 moles - 3.3 moles = 4.7 moles (to 1 decimal place)

pstnonsonjoku

The number of moles of excess reactant left unreacted is 4.67 moles

of Al.

The equation of the reaction is written as;

3Ag2S(s) +2Al-------> Al2S3(s) + 6Ag(s)

From the balanced reaction equation;

3 moles of Ag2S reacts with 2 moles of Al

5 moles of Ag2S reacts with x moles of Al

x = 5 moles × 2 moles /3 moles

x = 3.33 moles of Al

Hence, Al is the reactant in excess and Ag2S is the limiting reactant. The number of moles of excess reactant left unreacted is obtained from;

8 moles -  3.33 moles  = 4.67 moles

Learn more about stoichiometry: https://brainly.com/question/9743981

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