Respuesta :
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, [tex]Cu_2S[/tex] 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,
[tex]2Cu+S\rightarrow Cu_2S[/tex]
In this reaction, copper and sulfur are the reactants and copper sulfide is the product.
Let the mass of sulfur be 'x' gram
[tex]\text{The total mass of reactants}=\text{Total mass of copper}+\text{Total mass of sulfur}=2.54g+x[/tex]
[tex]\text{The total mass of product}=\text{Total mass of copper sulfide}=3.18g[/tex]
According to the law of conservation of mass,
[tex]\text{The total mass of reactants}=\text{The total mass of product}[/tex]
[tex]2.54g+x=3.18g[/tex]
[tex]x=(3.18-2.54)g[/tex]
[tex]x=0.64g[/tex]
Therefore, the total mass of sulfur consumed will be, 0.64 grams and the chemical formula of the compound produced is, [tex]Cu_2S[/tex] copper oxide.
