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In an experiment, 2.54 grams of copper completely reacts with sulfur, producing 3.18 grams of copper(I) sulfide.


Determine the total mass of sulfur consumed.

Write the chemical formula of the compound produced.

Verified Answer :

transitionstate

Answer:

               0.64 g of S


Solution:

               The balance chemical equation is as follow,


                                           2 Cu + S ----> Cu₂S


According to equation,


                        127 g (2 mole) Cu produces = 159 g (1 mole) of Cu₂S

So,

                                 2.54 g Cu will produce = X g of Cu₂S


Solving for X,

                     X = (2.54 g 159 g) / 127 g


                     X = 3.18 g of Cu₂S


Now, it is confirmed that the reaction is 100% ideal. Therefore,

As,


                       127 g (2 mole) Cu required = 32 g (1 mole) of S

So,

                                2.54 g Cu will require = X g of S


Solving for X,

                      X = (2.54 g 32 g) / 127 g


                      X = 0.64 g of S

Answer : The total mass of sulfur consumed will be, 0.64 grams and the chemical formula of the compound produced is, \(Cu_2S\) copper oxide.

Solution :

According to the law of conservation of mass, the total mass of reactant should be equal to the total mass of product.

The balanced chemical reaction will be,

\(2Cu+S\rightarrow Cu_2S\)

In this reaction, copper and sulfur are the reactants and copper sulfide is the product.

Let the mass of sulfur be 'x' gram

\(\text{The total mass of reactants}=\text{Total mass of copper}+\text{Total mass of sulfur}=2.54g+x\)

\(\text{The total mass of product}=\text{Total mass of copper sulfide}=3.18g\)

According to the law of conservation of mass,

\(\text{The total mass of reactants}=\text{The total mass of product}\)

\(2.54g+x=3.18g\)

\(x=(3.18-2.54)g\)

\(x=0.64g\)

Therefore, the total mass of sulfur consumed will be, 0.64 grams and the chemical formula of the compound produced is, \(Cu_2S\) copper oxide.

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