Assume That 8.5 L Of Iodine Gas \[$(I_2)\$\] Are Produced At STP According To The Equation:$\[ 2 \text{KI} (aq) + \text{Cl}_2 (g) \rightarrow 2 \text{KCl} (aq) + I_2 (g) \\]a. How Many Moles Of \[$I_2\$\] Are Produced?b. How

Feb 27, 2025 by ADMIN 225 views

**Production of Iodine Gas: Calculating Moles and Volume**

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Introduction

In this article, we will explore the production of iodine gas ( ${I_2}$ ) from the reaction between potassium iodide (KI) and chlorine gas (Cl2). The balanced chemical equation for this reaction is:

${ 2 \text{KI} (aq) + \text{Cl}_2 (g) \rightarrow 2 \text{KCl} (aq) + I_2 (g) }$

We will use this equation to calculate the number of moles of iodine gas produced and the volume of iodine gas at Standard Temperature and Pressure (STP).

Calculating Moles of Iodine Gas

To calculate the number of moles of iodine gas produced, we need to know the number of moles of reactants used. However, since we are given the volume of iodine gas produced, we can use the ideal gas law to calculate the number of moles.

The ideal gas law is given by:

${ PV = nRT }$

where:

${P}$ is the pressure in atmospheres (atm)
${V}$ is the volume in liters (L)
${n}$ is the number of moles
${R}$ is the gas constant (0.0821 L atm/mol K)
${T}$ is the temperature in Kelvin (K)

At STP, the pressure is 1 atm and the temperature is 273 K. We are given the volume of iodine gas produced as 8.5 L.

Step 1: Rearrange the Ideal Gas Law to Solve for n

To solve for the number of moles ( ${n}$ ), we need to rearrange the ideal gas law to isolate ${n}$ :

${ n = \frac{PV}{RT} }$

Step 2: Plug in the Values

Now, we can plug in the values into the equation:

${ n = \frac{(1 \text{ atm})(8.5 \text{ L})}{(0.0821 \text{ L atm/mol K})(273 \text{ K})} }$

Step 3: Calculate the Number of Moles

Now, we can calculate the number of moles:

${ n = \frac{(1)(8.5)}{(0.0821)(273)} }$ ${ n = \frac{8.5}{22.43} }$ ${ n = 0.38 \text{ mol} }$

Therefore, the number of moles of iodine gas produced is 0.38 mol.

Calculating Volume of Iodine Gas

To calculate the volume of iodine gas produced, we can use the ideal gas law again. However, this time, we are given the number of moles and we need to solve for the volume.

Step 1: Rearrange the Ideal Gas Law to Solve for V

To solve for the volume ( ${V}$ ), we need to rearrange the ideal gas law to isolate ${V}$ :

${ V = \frac{nRT}{P} }$

Step 2: Plug in the Values

Now, we can plug in the values into the equation:

${ V = \frac{(0.38 \text{ mol})(0.0821 \text{ L atm/mol K})(273 \text{ K})}{(1 \text{ atm})} }$

Step 3: Calculate the Volume

Now, we can calculate the volume:

${ V = \frac{(0.38)(0.0821)(273)}{1} }$ ${ V = \frac{9.31}{1} }$ ${ V = 9.31 \text{ L} }$

Therefore, the volume of iodine gas produced is 9.31 L.

Conclusion

In this article, we calculated the number of moles of iodine gas produced and the volume of iodine gas at STP using the ideal gas law. We found that the number of moles of iodine gas produced is 0.38 mol and the volume of iodine gas produced is 9.31 L.

References

Ideal Gas Law: The ideal gas law is a fundamental concept in chemistry that relates the pressure, volume, and temperature of a gas.
Standard Temperature and Pressure (STP): STP is a set of standard conditions for temperature and pressure that is used to measure the properties of gases.

Future Work

In the future, we can use this calculation to determine the yield of the reaction and to optimize the conditions for the production of iodine gas.

Limitations

One limitation of this calculation is that it assumes that the reaction is carried out at STP. In reality, the reaction may be carried out at different temperatures and pressures, which can affect the yield and properties of the product.

Conclusion

In conclusion, this article demonstrates how to calculate the number of moles of iodine gas produced and the volume of iodine gas at STP using the ideal gas law. This calculation is an important step in understanding the properties and behavior of gases and can be used to optimize the conditions for the production of iodine gas.

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Introduction

In our previous article, we explored the production of iodine gas ( ${I_2}$ ) from the reaction between potassium iodide (KI) and chlorine gas (Cl2). We calculated the number of moles of iodine gas produced and the volume of iodine gas at Standard Temperature and Pressure (STP) using the ideal gas law. In this article, we will answer some frequently asked questions (FAQs) related to the production of iodine gas.

Q: What is the balanced chemical equation for the production of iodine gas?

A: The balanced chemical equation for the production of iodine gas is:

${ 2 \text{KI} (aq) + \text{Cl}_2 (g) \rightarrow 2 \text{KCl} (aq) + I_2 (g) }$

Q: What is the ideal gas law and how is it used to calculate the number of moles of iodine gas produced?

A: The ideal gas law is a fundamental concept in chemistry that relates the pressure, volume, and temperature of a gas. It is given by:

${ PV = nRT }$

where:

${P}$ is the pressure in atmospheres (atm)
${V}$ is the volume in liters (L)
${n}$ is the number of moles
${R}$ is the gas constant (0.0821 L atm/mol K)
${T}$ is the temperature in Kelvin (K)

To calculate the number of moles of iodine gas produced, we can rearrange the ideal gas law to isolate ${n}$ :

${ n = \frac{PV}{RT} }$

Q: What is the volume of iodine gas produced at STP?

A: The volume of iodine gas produced at STP is 9.31 L.

Q: What are the limitations of this calculation?

A: One limitation of this calculation is that it assumes that the reaction is carried out at STP. In reality, the reaction may be carried out at different temperatures and pressures, which can affect the yield and properties of the product.

Q: How can the yield of the reaction be optimized?

A: The yield of the reaction can be optimized by adjusting the conditions of the reaction, such as the temperature, pressure, and concentration of the reactants.

Q: What are some potential applications of iodine gas?

A: Iodine gas has several potential applications, including:

Disinfection: Iodine gas can be used as a disinfectant to kill bacteria and other microorganisms.
Sterilization: Iodine gas can be used to sterilize medical equipment and other materials.
Water treatment: Iodine gas can be used to purify water by removing impurities and contaminants.

Q: What are some potential hazards associated with the production of iodine gas?

A: Some potential hazards associated with the production of iodine gas include:

Toxicity: Iodine gas can be toxic if inhaled or ingested in large quantities.
Corrosion: Iodine gas can corrode certain materials, such as metals and plastics.
Fire hazard: Iodine gas can be a fire hazard if it comes into contact with an ignition source.

Conclusion

In this article, we answered some frequently asked questions (FAQs) related to the production of iodine gas. We discussed the balanced chemical equation, the ideal gas law, and the limitations of the calculation. We also explored some potential applications and hazards associated with the production of iodine gas.