A Chemist Reacts Sodium Metal And Chlorine Gas To Form Salt According To The Balanced Chemical Equation: ${ 2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl} }$If The Chemist Has 35 G Of Na, What Mass Of Chlorine Must Be Used To React

Introduction

Chemical reactions are a fundamental aspect of chemistry, and understanding the principles behind them is crucial for chemists and scientists. One of the most common chemical reactions is the reaction between sodium metal and chlorine gas to form salt. This reaction is a classic example of a synthesis reaction, where two elements combine to form a compound. In this article, we will explore the balanced chemical equation for this reaction and use it to determine the mass of chlorine required to react with a given mass of sodium metal.

The Balanced Chemical Equation

The balanced chemical equation for the reaction between sodium metal and chlorine gas to form salt is:

${ 2 \text{Na} + \text{Cl}_2 \rightarrow 2 \text{NaCl} }$

This equation tells us that 2 moles of sodium metal react with 1 mole of chlorine gas to form 2 moles of sodium chloride (salt). The subscripts in the equation indicate the number of atoms of each element present in 1 mole of the compound.

Stoichiometry and Molar Ratios

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. In this case, the balanced chemical equation provides us with the molar ratios between sodium metal and chlorine gas. The molar ratio is the ratio of the number of moles of one substance to the number of moles of another substance.

From the balanced chemical equation, we can see that the molar ratio of sodium metal to chlorine gas is 2:1. This means that for every 2 moles of sodium metal, 1 mole of chlorine gas is required to react. This ratio is a fundamental concept in stoichiometry and is used to determine the amounts of reactants and products in chemical reactions.

Calculating the Mass of Chlorine Required

Now that we have the molar ratio between sodium metal and chlorine gas, we can use it to calculate the mass of chlorine required to react with a given mass of sodium metal. We are given that the chemist has 35 g of sodium metal. To calculate the mass of chlorine required, we need to follow these steps:

1. Determine the number of moles of sodium metal: We can use the molar mass of sodium metal (22.99 g/mol) to calculate the number of moles of sodium metal present in 35 g of the metal.

${ \text{Number of moles of Na} = \frac{\text{Mass of Na}}{\text{Molar mass of Na}} }$

${ \text{Number of moles of Na} = \frac{35 \text{ g}}{22.99 \text{ g/mol}} }$

${ \text{Number of moles of Na} = 1.52 \text{ mol} }$

2. Use the molar ratio to determine the number of moles of chlorine gas required: Since the molar ratio of sodium metal to chlorine gas is 2:1, we can use this ratio to determine the number of moles of chlorine gas required to react with 1.52 moles of sodium metal.

${ \text{Number of moles of Cl}_2 = \frac{\text{Number of moles of Na}}{2} }$

${ \text{Number of moles of Cl}_2 = \frac{1.52 \text{ mol}}{2} }$

${ \text{Number of moles of Cl}_2 = 0.76 \text{ mol} }$

3. Calculate the mass of chlorine gas required: We can use the molar mass of chlorine gas (70.90 g/mol) to calculate the mass of chlorine gas required to react with 0.76 moles of the gas.

${ \text{Mass of Cl}_2 = \text{Number of moles of Cl}_2 \times \text{Molar mass of Cl}_2 }$

${ \text{Mass of Cl}_2 = 0.76 \text{ mol} \times 70.90 \text{ g/mol} }$

${ \text{Mass of Cl}_2 = 53.88 \text{ g} }$

Therefore, the chemist must use 53.88 g of chlorine gas to react with 35 g of sodium metal.

Conclusion

In this article, we have explored the balanced chemical equation for the reaction between sodium metal and chlorine gas to form salt. We have used the molar ratio between sodium metal and chlorine gas to calculate the mass of chlorine required to react with a given mass of sodium metal. This calculation is a fundamental concept in stoichiometry and is used to determine the amounts of reactants and products in chemical reactions. By understanding the principles behind chemical reactions, chemists and scientists can design and optimize chemical processes to produce the desired products.

References

• CRC Handbook of Chemistry and Physics, 97th ed. (2016)
• Chemistry: An Atoms First Approach, 2nd ed. by Steven S. Zumdahl (2014)
• General Chemistry: Principles and Modern Applications, 11th ed. by Linus Pauling (2013)

Further Reading

• Chemical Reactions and Stoichiometry by OpenStax (2018)
• Chemical Reactions and Stoichiometry by Khan Academy (2020)
• Chemical Reactions and Stoichiometry by MIT OpenCourseWare (2019)
  

Introduction

In our previous article, we explored the balanced chemical equation for the reaction between sodium metal and chlorine gas to form salt. We also used the molar ratio between sodium metal and chlorine gas to calculate the mass of chlorine required to react with a given mass of sodium metal. In this article, we will answer some frequently asked questions (FAQs) related to this reaction.

Q: What is the purpose of the balanced chemical equation in this reaction?

A: The balanced chemical equation provides us with the molar ratios between reactants and products in a chemical reaction. In this case, the balanced chemical equation tells us that 2 moles of sodium metal react with 1 mole of chlorine gas to form 2 moles of sodium chloride (salt).

Q: Why is the molar ratio between sodium metal and chlorine gas important?

A: The molar ratio between sodium metal and chlorine gas is crucial in determining the amounts of reactants and products in a chemical reaction. By knowing the molar ratio, we can calculate the mass of chlorine required to react with a given mass of sodium metal.

Q: How do we calculate the mass of chlorine required to react with a given mass of sodium metal?

A: To calculate the mass of chlorine required, we need to follow these steps:

1. Determine the number of moles of sodium metal present in the given mass of the metal.
2. Use the molar ratio to determine the number of moles of chlorine gas required to react with the given number of moles of sodium metal.
3. Calculate the mass of chlorine gas required to react with the given number of moles of chlorine gas.

Q: What is the molar mass of sodium metal and chlorine gas?

A: The molar mass of sodium metal is 22.99 g/mol, and the molar mass of chlorine gas is 70.90 g/mol.

Q: How do we determine the number of moles of sodium metal present in a given mass of the metal?

A: We can use the formula:

${ \text{Number of moles of Na} = \frac{\text{Mass of Na}}{\text{Molar mass of Na}} }$

Q: What is the significance of the balanced chemical equation in stoichiometry?

A: The balanced chemical equation is a fundamental concept in stoichiometry, which deals with the quantitative relationships between reactants and products in chemical reactions. By understanding the balanced chemical equation, we can design and optimize chemical processes to produce the desired products.

Q: Can we use the balanced chemical equation to predict the products of a chemical reaction?

A: Yes, the balanced chemical equation can be used to predict the products of a chemical reaction. By analyzing the reactants and products in the balanced chemical equation, we can determine the products of a chemical reaction.

Q: How do we balance a chemical equation?

A: To balance a chemical equation, we need to ensure that the number of atoms of each element is the same on both the reactant and product sides of the equation. We can use the following steps to balance a chemical equation:

1. Write the unbalanced chemical equation.
2. Count the number of atoms of each element on both the reactant and product sides of the equation.
3. Add coefficients to the reactants and products to ensure that the number of atoms of each element is the same on both sides of the equation.

Q: What is the difference between a balanced chemical equation and an unbalanced chemical equation?

A: A balanced chemical equation is an equation in which the number of atoms of each element is the same on both the reactant and product sides of the equation. An unbalanced chemical equation is an equation in which the number of atoms of each element is not the same on both the reactant and product sides of the equation.

Q: Can we use the balanced chemical equation to determine the limiting reactant in a chemical reaction?

A: Yes, the balanced chemical equation can be used to determine the limiting reactant in a chemical reaction. By analyzing the reactants and products in the balanced chemical equation, we can determine which reactant is the limiting reactant.

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

A: To determine the limiting reactant in a chemical reaction, we need to follow these steps:

1. Write the balanced chemical equation for the reaction.
2. Determine the number of moles of each reactant present in the reaction.
3. Use the molar ratio between the reactants to determine which reactant is the limiting reactant.

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

A: The limiting reactant is the reactant that is consumed first in a chemical reaction. By understanding the limiting reactant, we can design and optimize chemical processes to produce the desired products.

Conclusion

In this article, we have answered some frequently asked questions (FAQs) related to the reaction between sodium metal and chlorine gas to form salt. We have discussed the importance of the balanced chemical equation, the molar ratio between sodium metal and chlorine gas, and the calculation of the mass of chlorine required to react with a given mass of sodium metal. By understanding the principles behind chemical reactions, chemists and scientists can design and optimize chemical processes to produce the desired products.

References

• CRC Handbook of Chemistry and Physics, 97th ed. (2016)
• Chemistry: An Atoms First Approach, 2nd ed. by Steven S. Zumdahl (2014)
• General Chemistry: Principles and Modern Applications, 11th ed. by Linus Pauling (2013)

Further Reading

• Chemical Reactions and Stoichiometry by OpenStax (2018)
• Chemical Reactions and Stoichiometry by Khan Academy (2020)
• Chemical Reactions and Stoichiometry by MIT OpenCourseWare (2019)