Volume Calculation for Hydrochloric Acid Production from Hydrogen and Chlorine

The production of hydrochloric acid (HCl) involves an exothermic reaction between hydrogen (H?) and chlorine (Cl?). The balanced chemical equation for this reaction is:

H? Cl? ? 2HCl

The problem involves determining the volume of hydrogen required to produce 10 liters of HCl gas under Volume Calculation for Hydrochloric Acid Production from Hydrogen and Chlorine

The production of hydrochloric acid (HCl) involves an exothermic reaction between hydrogen (H?) and chlorine (Cl?). The balanced chemical equation for this reaction is:

H? Cl? ? 2HCl

The problem involves determining the volume of hydrogen required to produce 10 liters of HCl gas under standard pressure and temperature (STP). At STP, one mole of any gas occupies 22.414 liters. This value is crucial for converting between volume and moles of gas in the calculations for chemical reactions involving gases.

Step-by-Step Explanation

To solve this problem, follow these steps:

Identify the given information: Volume of HCl gas required 10 liters. Use the ideal gas law for volume calculations: At STP, one mole of gas occupies 22.414 liters (molar volume).

Calculation Process

The molar volume (V) at standard conditions is given by the equation:

V n × 22.414 L

Where n is the number of moles of gas.

The balanced chemical equation shows that 1 mole of H? reacts with 1 mole of Cl? to produce 2 moles of HCl. Thus, to produce 10 liters of HCl, we need to calculate the equivalent volume of H? required.

Step 1: Calculate Moles of HCl

Using the molar volume constant:

n[HCl] 10 liters / 22.414 liters/mole

n[HCl] ≈ 0.4459 moles

Step 2: Calculate Moles of H?

From the balanced equation H? Cl? ? 2HCl, we see that 1 mole of H? produces 2 moles of HCl. Therefore:

n[H?] n[HCl] / 2

n[H?] 0.4459 moles / 2

n[H?] ≈ 0.22295 moles

Step 3: Calculate Volume of H?

Using the molar volume constant again:

V[H?] n[H?] × 22.414 liters/mole

V[H?] 0.22295 moles × 22.414 liters/mole

V[H?] ≈ 5 liters

Conclusion

To produce 10 liters of HCl gas at STP, approximately 5 liters of hydrogen gas (H?) are required.

Additional Notes

This problem demonstrates the application of the ideal gas law and molar volume constants in chemical reaction stoichiometry. Understanding these concepts is crucial for solving problems in chemistry, particularly those involving gas laws and chemical reactions between gases.

Other Relevant Applications

The principles used in this calculation are applicable in various fields, including:

Environmental science: Monitoring and controlling industrial emissions involving HCl. Material science: Understanding gas phase reactions in the synthesis of nanoparticles and other materials. Energy: Chlorination processes in water treatment and cleaning of industrial gases.