What is the balanced chemical equation for the reaction involving CuO and H₂?

The balanced equation is CuO(s) + H₂(g) → Cu(s) + H₂O(g).

How many moles of hydrogen gas are used if 250 L are provided at standard temperature and pressure (STP)?

At STP, 1 mol of gas occupies 22.4 L. Therefore, 250 L of H₂ corresponds to approximately 11.16 moles (250 ÷ 22.4).

What is the theoretical mass of copper metal produced from 250 L of hydrogen gas?

Using 11.16 mol of H₂, which reacts in a 1:1 ratio to produce 11.16 mol of Cu, the mass of Cu produced is 11.16 mol × 63.55 g/mol ≈ 710.5 grams.

How would the reaction shift if excess CuO is present?

If excess CuO is present, the reaction will proceed until all H₂ is consumed, producing maximum Cu and H₂O, with the limiting reagent being H₂.

What are the key factors influencing the reaction efficiency in this process?

Factors include temperature, pressure, purity of reactants, and surface area of CuO, which all affect reaction rate and completeness.

How can this reaction be utilized in industrial hydrogen production or metal extraction?

This reaction can be used in processes like copper ore reduction, where hydrogen acts as a reducing agent to produce pure copper, or in hydrogen storage systems.

What safety precautions should be taken when handling hydrogen gas in this reaction?

Hydrogen is flammable and explosive; proper ventilation, avoiding sparks or open flames, and using appropriate containment are essential safety measures.

Given The Following Reaction: CuO (s) + H2 (g) Cu (s) + H2O (g) If 250. L Of Hydrogen Gas Are Used To

Given The Following Reaction: CuO (s) + H2 (g) Cu (s) + H2O (g) If 250. L Of Hydrogen Gas Are Used To analyze the chemical process, it is essential to understand the fundamentals of the reaction, the stoichiometry involved, and the practical applications of this chemical transformation. This reaction exemplifies a reduction process where copper(II) oxide (CuO) reacts with hydrogen gas (H2) to produce metallic copper (Cu) and water vapor (H2O). In this article, we will delve into the details of this reaction, explore the calculations involved in quantifying reactants and products, and discuss its significance in industrial and laboratory settings.

Understanding the Reaction: CuO and Hydrogen Gas

Reaction Overview

This chemical reaction is a classic example of a reduction-oxidation (redox) process. Copper(II) oxide (CuO) acts as an oxidizing agent, accepting electrons from hydrogen gas, which serves as the reducing agent. The overall reaction can be written as:

CuO (s) + H2 (g) → Cu (s) + H2O (g)

In this process, solid copper metal is produced alongside water vapor, which may be in gaseous form depending on temperature and pressure conditions.

Significance of the Reaction

This reaction is vital in several contexts:

Metallurgical processes: Extracting pure copper from its oxide ore.
Laboratory synthesis: Demonstrating redox reactions and stoichiometry.
Industrial applications: Producing copper metal and water vapor in controlled environments.

Calculating the Moles of Hydrogen Gas Used

Given Volume and Conditions

The problem states that 250 liters of hydrogen gas are used. To perform calculations accurately, assumptions about temperature and pressure are necessary, typically assuming standard temperature and pressure (STP), where:

Temperature = 273.15 K
Pressure = 1 atm
1 mol of gas occupies 22.4 liters at STP

Converting Volume to Moles

Using the molar volume at STP:

Number of moles of H2 = Volume of H2 / Molar volume
= 250 L / 22.4 L/mol
≈ 11.16 mol

This means approximately 11.16 moles of hydrogen gas are involved in the reaction.

Stoichiometry of the Reaction

Balanced Chemical Equation

The reaction is already balanced:

CuO (s) + H2 (g) → Cu (s) + H2O (g)

This indicates a 1:1 molar ratio between CuO and H2, and between H2 and H2O.

Reactant and Product Quantities

For every 1 mol of H2 consumed, 1 mol of CuO reacts.
The amount of water produced correlates directly with hydrogen consumption.

Given the moles of H2 (≈11.16 mol), the reaction would theoretically consume an equal amount of CuO and produce the same amount of water vapor.

Mass and Volume Calculations

Mass of Copper Produced

Using molar mass:

Molar mass of Cu = 63.55 g/mol

Mass of Cu produced: = 11.16 mol × 63.55 g/mol ≈ 709.8 g

This indicates that approximately 709.8 grams of metallic copper can be produced from 250 L of hydrogen gas under the specified conditions.

Volume of Water Vapor Produced

Since water is produced as a gas (H2O vapor), and assuming ideal gas behavior at STP:

Volume of H2O vapor = moles of H2O × molar volume
= 11.16 mol × 22.4 L/mol
≈ 250 L

Thus, the reaction produces approximately 250 liters of water vapor, matching the volume of hydrogen used, assuming all hydrogen is consumed.

Practical Applications and Industrial Relevance

Metallurgical Extraction of Copper

This reaction is fundamental in the smelting and refining of copper ores. Copper oxides are reduced to metallic copper using hydrogen, which is a cleaner alternative to carbon reduction methods, reducing sulfur dioxide emissions.

Hydrogen as a Reducing Agent

Hydrogen gas offers several advantages:

Produces water instead of greenhouse gases like CO2.
Enables pure copper recovery.
Suitable for environmentally friendly metal extraction processes.

Laboratory and Educational Uses

This reaction serves as an excellent demonstration of redox chemistry, stoichiometry, and gas-volume relationships at STP.

Additional Considerations

Reaction Conditions

Temperature: Elevated temperatures favor the reduction process.
Pressure: Increased pressure can influence gas volumes and reaction rates.
Purity of reactants: Impurities can affect reaction efficiency.

Limitations and Safety

Hydrogen gas is flammable and requires careful handling.
Proper ventilation and safety protocols are necessary during experiments or industrial operations.

Summary and Conclusion

Analyzing the reaction between copper(II) oxide and hydrogen gas reveals how stoichiometry and gas laws interplay to determine reactant and product quantities. Using 250 liters of hydrogen gas at STP corresponds to roughly 11.16 moles, which theoretically produces about 709.8 grams of copper and 250 liters of water vapor. This process exemplifies efficient reduction techniques crucial in metal extraction industries, highlighting the importance of chemical calculations in practical applications.

In conclusion, understanding the quantitative aspects of this redox reaction enables chemists and engineers to optimize processes, predict yields, and design environmentally friendly methods for metal recovery. The reaction's simplicity, combined with its industrial significance, underscores the central role of stoichiometry and gas laws in modern chemistry.