Copper Reacts With Sulfur To Form Copper (I) Sulfide, According To The Balanced Equation Below:${ 2 \text{Cu} + \text{S} \rightarrow \text{Cu}_2\text{S} }$Given That There Are 40.2 G Cu And 14.1 G S, Complete The Steps Below To Determine The

Copper Reacts with Sulfur: A Step-by-Step Guide to Balancing Chemical Equations and Determining Limiting Reactants

Chemical reactions are the foundation of chemistry, and understanding how they work is crucial for predicting the outcomes of various processes. In this article, we will explore the reaction between copper (Cu) and sulfur (S) to form copper (I) sulfide (Cu2S). We will start by writing the balanced chemical equation and then use the given masses of Cu and S to determine the limiting reactant.

Writing the Balanced Chemical Equation

The balanced chemical equation for the reaction between copper and sulfur is:

${ 2 \text{Cu} + \text{S} \rightarrow \text{Cu}_2\text{S} }$

This equation indicates that 2 moles of copper react with 1 mole of sulfur to produce 1 mole of copper (I) sulfide.

Determining the Molar Masses of Cu and S

To proceed with the calculation, we need to determine the molar masses of Cu and S. The atomic masses of Cu and S are 63.55 g/mol and 32.07 g/mol, respectively.

Calculating the Number of Moles of Cu and S

We are given the masses of Cu and S as 40.2 g and 14.1 g, respectively. We can use the molar masses to calculate the number of moles of each substance:

${ \text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} = \frac{40.2 \text{ g}}{63.55 \text{ g/mol}} = 0.633 \text{ mol} }$

${ \text{moles of S} = \frac{\text{mass of S}}{\text{molar mass of S}} = \frac{14.1 \text{ g}}{32.07 \text{ g/mol}} = 0.439 \text{ mol} }$

Determining the Limiting Reactant

The balanced chemical equation indicates that 2 moles of Cu react with 1 mole of S. We can use the mole ratios to determine the limiting reactant:

${ \text{Cu}: \text{S} = 2:1 }$

We can calculate the number of moles of Cu required to react with 0.439 mol of S:

${ \text{moles of Cu required} = 2 \times \text{moles of S} = 2 \times 0.439 \text{ mol} = 0.878 \text{ mol} }$

Since we have only 0.633 mol of Cu, which is less than the required 0.878 mol, Cu is the limiting reactant.

Calculating the Mass of Cu2S Produced

Now that we have determined the limiting reactant, we can calculate the mass of Cu2S produced. The molar mass of Cu2S is 159.16 g/mol. We can use the number of moles of Cu to calculate the mass of Cu2S produced:

${ \text{mass of Cu2S produced} = \text{moles of Cu} \times \text{molar mass of Cu2S} = 0.633 \text{ mol} \times 159.16 \text{ g/mol} = 100.7 \text{ g} }$

In this article, we have explored the reaction between copper and sulfur to form copper (I) sulfide. We have written the balanced chemical equation, determined the molar masses of Cu and S, calculated the number of moles of each substance, determined the limiting reactant, and calculated the mass of Cu2S produced. This example illustrates the importance of understanding chemical reactions and balancing equations in chemistry.

Limitations and Future Directions

While this example has provided a clear understanding of the reaction between copper and sulfur, there are several limitations and future directions to consider. For instance, the reaction may not be as straightforward in real-world scenarios, and other factors such as temperature, pressure, and catalysts may affect the outcome. Additionally, the calculation of the mass of Cu2S produced assumes that the reaction is 100% efficient, which may not be the case in reality. Future research could focus on exploring the effects of these factors on the reaction and developing more accurate models for predicting the outcomes of chemical reactions.

• [1] Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General chemistry: Principles and modern applications. Pearson Prentice Hall.
• [2] Atkins, P. W., & De Paula, J. (2006). Physical chemistry. Oxford University Press.

The following table summarizes the calculations performed in this article:

Substance	Mass (g)	Molar Mass (g/mol)	Moles	Limiting Reactant
Cu	40.2	63.55	0.633	Yes
S	14.1	32.07	0.439	No

Note: The table is not exhaustive and only includes the substances and calculations relevant to this article.
Copper Reacts with Sulfur: A Q&A Guide to Balancing Chemical Equations and Determining Limiting Reactants

In our previous article, we explored the reaction between copper (Cu) and sulfur (S) to form copper (I) sulfide (Cu2S). We wrote the balanced chemical equation, determined the molar masses of Cu and S, calculated the number of moles of each substance, determined the limiting reactant, and calculated the mass of Cu2S produced. In this article, we will answer some frequently asked questions (FAQs) related to this topic.

Q: What is the balanced chemical equation for the reaction between copper and sulfur?

A: The balanced chemical equation for the reaction between copper and sulfur is:

${ 2 \text{Cu} + \text{S} \rightarrow \text{Cu}_2\text{S} }$

Q: What is the molar mass of copper (Cu)?

A: The molar mass of copper (Cu) is 63.55 g/mol.

Q: What is the molar mass of sulfur (S)?

A: The molar mass of sulfur (S) is 32.07 g/mol.

Q: How do I calculate the number of moles of copper (Cu) and sulfur (S) given their masses?

A: To calculate the number of moles of copper (Cu) and sulfur (S), you can use the following formulas:

${ \text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} }$

${ \text{moles of S} = \frac{\text{mass of S}}{\text{molar mass of S}} }$

Q: How do I determine the limiting reactant in a chemical reaction?

A: To determine the limiting reactant, you can compare the mole ratio of the reactants to the coefficients in the balanced chemical equation. The reactant with the smaller mole ratio is the limiting reactant.

Q: How do I calculate the mass of the product (Cu2S) produced in a chemical reaction?

A: To calculate the mass of the product (Cu2S) produced, you can use the following formula:

${ \text{mass of Cu2S} = \text{moles of Cu} \times \text{molar mass of Cu2S} }$

Q: What is the significance of the limiting reactant in a chemical reaction?

A: The limiting reactant is the reactant that determines the amount of product that can be formed in a chemical reaction. It is the reactant that is consumed first and is responsible for limiting the amount of product that can be formed.

Q: Can I use this method to determine the limiting reactant in any chemical reaction?

A: No, this method is only applicable to chemical reactions where the mole ratio of the reactants is known and the balanced chemical equation is available. In some cases, the mole ratio of the reactants may not be known, and other methods such as the method of initial rates may be used to determine the limiting reactant.

In this article, we have answered some frequently asked questions related to the reaction between copper and sulfur to form copper (I) sulfide. We have provided a step-by-step guide to balancing chemical equations, determining the molar masses of reactants, calculating the number of moles of reactants, determining the limiting reactant, and calculating the mass of the product produced. This article is a useful resource for students and professionals who want to understand the basics of chemical reactions and balancing equations.

• [1] Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2006). General chemistry: Principles and modern applications. Pearson Prentice Hall.
• [2] Atkins, P. W., & De Paula, J. (2006). Physical chemistry. Oxford University Press.

The following table summarizes the calculations performed in this article:

Substance	Mass (g)	Molar Mass (g/mol)	Moles	Limiting Reactant
Cu	40.2	63.55	0.633	Yes
S	14.1	32.07	0.439	No

Note: The table is not exhaustive and only includes the substances and calculations relevant to this article.