Balanced equation of reaction of copper and sulfur 1) are given below. 2Cu (s) +

Question

Balanced equation of reaction of copper and sulfur 1) are given below. 2Cu (s) +S (s) Cu2S (s) a) In the above reaction, 1.890 g of Cu was reacted with 0.238 g of sulfur(S). .Calculate the limiting reactant. Show setup with conversion factors and finish with c.v. and f.v. If do not use correct conversion factors steps, points will be deducted. Show calculation as srep1, 2, 3 etc Limiting reactant of product formed mole b) Calculate the mass of product formed, Show setup with conversion factors and finish with c.v. and f.v.If do not use correct conversion factors steps, points will be deducted

Explanation / Answer

Since, the balanced equation is already given,

2 Cu (s) + S (s) ? Cu2S (s)

a) We'll start be calculating the no. of grams of sulphur required for reacting 1.890 gm of copper.

the theoritical yield of the S (s) = ?

= (1.890 g of Cu) * (1 mol of Cu / 63.55 g ) * (1 mol of S / 2 mol of Cu) *( 32.06 g / 1 mol of S)

= 0.476 g of Sulphur.

If you reacted all the (1.890 g) of copper , you will need to use 0.476 g of sulphur. Hence, Sulphur is the limiting reactant here cause we are given only, 0.238 g of sulphur. After reacting 0.238 g of sulphur still some amount of copper will be left.

b) the mass of product formed can be calculated in the same manner, as below

= (1.890 g of Cu) * (1 mol of Cu / 63.55 g ) * (1 mol of Cu2S / 2 mol of Cu) *( 159.16 g / 1 mol of Cu2S)

= 2.367 g of Cu2S will be formed.

I hope this helps!

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