Answer:
The mass of copper(II) sulfide formed is:
= 81.24 g
Explanation:
The Balanced chemical equation for this reaction is :
![Cu(s) + S\rightarrow CuS](https://tex.z-dn.net/?f=Cu%28s%29%20%2B%20S%5Crightarrow%20CuS)
given mass= 54 g
Molar mass of Cu = 63.55 g/mol
![Moles = \frac{given\ mass}{Molar\ mass}](https://tex.z-dn.net/?f=Moles%20%3D%20%5Cfrac%7Bgiven%5C%20mass%7D%7BMolar%5C%20mass%7D)
Moles of Cu = 0.8497 mol
Given mass = 42 g
Molar mass of S = 32.06 g/mol
![Moles = \frac{given\ mass}{Molar\ mass}](https://tex.z-dn.net/?f=Moles%20%3D%20%5Cfrac%7Bgiven%5C%20mass%7D%7BMolar%5C%20mass%7D)
Moles of S = 1.31 mol
Limiting Reagent :<em> The reagent which is present in less amount and consumed in a reactio</em>n
<u><em>First find the limiting reagent :</em></u>
![Cu + S\rightarrow CuS](https://tex.z-dn.net/?f=Cu%20%2B%20S%5Crightarrow%20CuS)
1 mol of Cu require = 1 mol of S
0.8497 mol of Cu should require = 1 x 0.8497 mol
= 0.8497 mol of S
S present in the reaction Medium = 1.31 mol
S Required = 0.8497 mol
S is present in excess and <u>Cu is limiting reagent</u>
<u>All Cu is consumed in the reaction</u>
Amount Cu will decide the amount of CuS formed
![Cu + S\rightarrow CuS](https://tex.z-dn.net/?f=Cu%20%2B%20S%5Crightarrow%20CuS)
1 mole of Cu gives = 1 mole of Copper sulfide
0.8497 mol of Cu = 1 x 0.8497 mole of Copper sulfide
= 0.8497
Molar mass of CuS = 95.611 g/mol
![Moles = \frac{given\ mass}{Molar\ mass}](https://tex.z-dn.net/?f=Moles%20%3D%20%5Cfrac%7Bgiven%5C%20mass%7D%7BMolar%5C%20mass%7D)
![0.8497 = \frac{given\ mass}{95.611}](https://tex.z-dn.net/?f=0.8497%20%3D%20%5Cfrac%7Bgiven%5C%20mass%7D%7B95.611%7D)
Mass of CuS = 0.8497 x 95.611
= 81.24 g