In The Reaction C + O 2 → C O 2 C + O_2 \rightarrow CO_2 C + O 2 ​ → C O 2 ​ , 18 G Of Carbon React With Oxygen To Produce 72 G Of Carbon Dioxide. What Mass Of Oxygen Would Be Needed In The Reaction?A. 18 G B. 54 G C. 72 G D. 90 G

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Understanding the Chemical Reaction

In the given reaction, carbon (C) reacts with oxygen (O2) to produce carbon dioxide (CO2). The reaction is as follows:

C + O2 → CO2

Given Information

  • 18 g of carbon (C) react with oxygen to produce 72 g of carbon dioxide (CO2).

Objective

To determine the mass of oxygen (O2) needed in the reaction.

Step 1: Write Down the Balanced Chemical Equation

To solve this problem, we need to write down the balanced chemical equation for the reaction. The balanced equation is:

2C + O2 → 2CO2

Step 2: Identify the Molar Masses

To proceed with the calculation, we need to identify the molar masses of carbon (C) and oxygen (O2). The molar masses are:

  • C: 12 g/mol
  • O2: 32 g/mol

Step 3: Calculate the Number of Moles of Carbon

Using the given mass of carbon (18 g), we can calculate the number of moles of carbon:

moles C = mass C / molar mass C moles C = 18 g / 12 g/mol moles C = 1.5 mol

Step 4: Calculate the Number of Moles of Carbon Dioxide

Using the given mass of carbon dioxide (72 g), we can calculate the number of moles of carbon dioxide:

moles CO2 = mass CO2 / molar mass CO2 moles CO2 = 72 g / (44 g/mol) moles CO2 = 1.636 mol

Step 5: Calculate the Number of Moles of Oxygen

From the balanced chemical equation, we can see that 1 mole of O2 produces 2 moles of CO2. Therefore, the number of moles of O2 required to produce 1.636 mol of CO2 is:

moles O2 = moles CO2 / 2 moles O2 = 1.636 mol / 2 moles O2 = 0.818 mol

Step 6: Calculate the Mass of Oxygen

Using the number of moles of oxygen (0.818 mol) and the molar mass of oxygen (32 g/mol), we can calculate the mass of oxygen:

mass O2 = moles O2 x molar mass O2 mass O2 = 0.818 mol x 32 g/mol mass O2 = 26.176 g

Conclusion

Therefore, the mass of oxygen needed in the reaction is approximately 26.176 g.

Answer

The correct answer is not listed in the options provided. However, based on our calculation, the mass of oxygen needed in the reaction is approximately 26.176 g.

Discussion

This problem requires a good understanding of chemical equations, stoichiometry, and molar masses. The balanced chemical equation is essential in solving this problem. By identifying the molar masses of carbon and oxygen, we can calculate the number of moles of carbon and carbon dioxide. Then, we can use the balanced chemical equation to calculate the number of moles of oxygen required. Finally, we can calculate the mass of oxygen using the number of moles and the molar mass.

Key Takeaways

  • Balancing chemical equations is essential in solving stoichiometry problems.
  • Molar masses are crucial in calculating the number of moles of a substance.
  • Stoichiometry involves calculating the amount of substance required or produced in a chemical reaction.

Additional Resources

For more information on balancing chemical equations and stoichiometry, please refer to the following resources:

Q1: What is the difference between a balanced chemical equation and an unbalanced chemical equation?

A1: 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. 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.

Q2: How do I balance a chemical equation?

A2: To balance a chemical equation, you need to add coefficients in front of the formulas of the reactants or products to make the number of atoms of each element the same on both sides. You can start by balancing the elements that appear only once on each side, and then balance the elements that appear multiple times.

Q3: What is the law of conservation of mass?

A3: The law of conservation of mass states that matter cannot be created or destroyed in a chemical reaction. This means that the total mass of the reactants must be equal to the total mass of the products.

Q4: What is stoichiometry?

A4: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves calculating the amount of substance required or produced in a chemical reaction.

Q5: How do I calculate the number of moles of a substance?

A5: To calculate the number of moles of a substance, you need to divide the mass of the substance by its molar mass. The molar mass is the mass of one mole of the substance.

Q6: What is the difference between a mole and a gram?

A6: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules). A gram is a unit of mass that represents 1/1000 of a kilogram.

Q7: How do I calculate the mass of a substance from its number of moles?

A7: To calculate the mass of a substance from its number of moles, you need to multiply the number of moles by the molar mass of the substance.

Q8: What is the significance of molar mass in stoichiometry?

A8: Molar mass is a crucial concept in stoichiometry because it allows us to calculate the number of moles of a substance from its mass, and vice versa.

Q9: How do I determine the limiting reactant in a chemical reaction?

A9: To determine the limiting reactant in a chemical reaction, you need to compare the mole ratio of the reactants to the mole ratio of the products. The reactant that is present in the smallest amount is the limiting reactant.

Q10: What is the difference between a reactant and a product in a chemical reaction?

A10: A reactant is a substance that is consumed in a chemical reaction, while a product is a substance that is formed in a chemical reaction.

Conclusion

Balancing chemical equations and stoichiometry are essential concepts in chemistry that help us understand the quantitative relationships between reactants and products in a chemical reaction. By understanding these concepts, we can calculate the amount of substance required or produced in a chemical reaction, and determine the limiting reactant in a chemical reaction.

Additional Resources

For more information on balancing chemical equations and stoichiometry, please refer to the following resources: