How Many Grams Of Oxygen Are Needed To React With 160 G Of Hydrazine? Express Your Answer To Three Significant Figures And Include The Appropriate Units.${ M = }$Value: __________Units: __________
Introduction
Chemical reactions involve the transformation of one or more substances into new substances. These reactions are governed by the laws of conservation of mass and energy. In this article, we will delve into the world of stoichiometry, which is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. We will explore how to balance chemical equations and calculate the amount of oxygen needed to react with a given amount of hydrazine.
Understanding the Chemical Reaction
The chemical reaction we will be focusing on is the combustion of hydrazine (N2H4) in the presence of oxygen (O2). The balanced chemical equation for this reaction is:
2N2H4 + 5O2 → 4N2 + 8H2O
In this equation, 2 moles of hydrazine react with 5 moles of oxygen to produce 4 moles of nitrogen gas and 8 moles of water.
Calculating the Amount of Oxygen Needed
To calculate the amount of oxygen needed to react with 160 g of hydrazine, we need to follow these steps:
- Determine the molar mass of hydrazine: The molar mass of hydrazine (N2H4) is 32.05 g/mol.
- Calculate the number of moles of hydrazine: We can calculate the number of moles of hydrazine using the formula:
moles = mass / molar mass
moles = 160 g / 32.05 g/mol = 5.00 mol
- Determine the mole ratio of hydrazine to oxygen: From the balanced chemical equation, we can see that 2 moles of hydrazine react with 5 moles of oxygen. Therefore, the mole ratio of hydrazine to oxygen is 2:5 or 0.4:1.
- Calculate the number of moles of oxygen needed: We can calculate the number of moles of oxygen needed using the mole ratio:
moles of oxygen = moles of hydrazine x mole ratio moles of oxygen = 5.00 mol x 0.4 = 2.00 mol
- Determine the molar mass of oxygen: The molar mass of oxygen (O2) is 32.00 g/mol.
- Calculate the mass of oxygen needed: We can calculate the mass of oxygen needed using the formula:
mass = moles x molar mass
mass = 2.00 mol x 32.00 g/mol = 64.00 g
Therefore, 64.0 g of oxygen are needed to react with 160 g of hydrazine.
Conclusion
In this article, we have explored the concept of stoichiometry and how to balance chemical equations. We have also calculated the amount of oxygen needed to react with 160 g of hydrazine. By following the steps outlined in this article, you can calculate the amount of reactants needed to produce a given amount of products in any chemical reaction.
Additional Resources
- Balancing Chemical Equations: A comprehensive guide to balancing chemical equations.
- Stoichiometry: A branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions.
- Molar Mass: The mass of one mole of a substance.
References
- CRC Handbook of Chemistry and Physics: A comprehensive reference book that provides the molar masses of various substances.
- Chemical Equations: A website that provides a comprehensive guide to balancing chemical equations.
Discussion
- What is stoichiometry?
- How do you balance a chemical equation?
- What is the molar mass of oxygen?
Answer Key
- What is the amount of oxygen needed to react with 160 g of hydrazine?
- 64.0 g
- What is the molar mass of hydrazine?
- 32.05 g/mol
- What is the mole ratio of hydrazine to oxygen?
- 2:5 or 0.4:1
Frequently Asked Questions: Stoichiometry and Balancing Chemical Equations ====================================================================
Q: What is stoichiometry?
A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves calculating the amount of reactants needed to produce a given amount of products.
Q: How do I balance a chemical equation?
A: Balancing a chemical equation involves ensuring that the number of atoms of each element is the same on both the reactant and product sides of the equation. This can be done by adding coefficients (numbers in front of the formulas of reactants or products) to balance the equation.
Q: What is the molar mass of oxygen?
A: The molar mass of oxygen (O2) is 32.00 g/mol.
Q: How do I calculate the amount of oxygen needed to react with a given amount of hydrazine?
A: To calculate the amount of oxygen needed to react with a given amount of hydrazine, you need to follow these steps:
- Determine the molar mass of hydrazine.
- Calculate the number of moles of hydrazine.
- Determine the mole ratio of hydrazine to oxygen.
- Calculate the number of moles of oxygen needed.
- Determine the molar mass of oxygen.
- Calculate the mass of oxygen needed.
Q: What is the mole ratio of hydrazine to oxygen?
A: The mole ratio of hydrazine to oxygen is 2:5 or 0.4:1.
Q: How do I calculate the number of moles of oxygen needed?
A: To calculate the number of moles of oxygen needed, you can use the mole ratio:
moles of oxygen = moles of hydrazine x mole ratio
Q: What is the molar mass of hydrazine?
A: The molar mass of hydrazine (N2H4) is 32.05 g/mol.
Q: How do I calculate the mass of oxygen needed?
A: To calculate the mass of oxygen needed, you can use the formula:
mass = moles x molar mass
Q: What is the amount of oxygen needed to react with 160 g of hydrazine?
A: The amount of oxygen needed to react with 160 g of hydrazine is 64.0 g.
Q: What is the difference between a balanced and unbalanced chemical equation?
A: A balanced chemical equation has the same number of atoms of each element on both the reactant and product sides of the equation. An unbalanced chemical equation does not have the same number of atoms of each element on both sides.
Q: How do I determine the mole ratio of reactants to products in a chemical reaction?
A: To determine the mole ratio of reactants to products in a chemical reaction, you need to balance the chemical equation and then use the coefficients to determine the mole ratio.
Q: What is the importance of stoichiometry in chemistry?
A: Stoichiometry is important in chemistry because it allows us to calculate the amount of reactants needed to produce a given amount of products. This is essential in many fields, including chemistry, biology, and engineering.
Q: How do I apply stoichiometry in real-life situations?
A: Stoichiometry can be applied in many real-life situations, such as:
- Calculating the amount of reactants needed to produce a given amount of products in a chemical reaction.
- Determining the amount of oxygen needed to support combustion reactions.
- Calculating the amount of reactants needed to produce a given amount of products in a biological reaction.
Conclusion
In this article, we have answered some of the most frequently asked questions about stoichiometry and balancing chemical equations. We have also provided examples and explanations to help you understand the concepts better. By applying the principles of stoichiometry, you can calculate the amount of reactants needed to produce a given amount of products in any chemical reaction.