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Oct 13, 2025 by orovajewels.com 29 views

Understanding the Decomposition Reaction of NOBr(g)

The decomposition reaction of NOBr(g) is a complex process that involves the breakdown of a single compound into two simpler substances. In this case, the reaction is represented by the equation:

$\operatorname{NOBr}(g) \rightleftharpoons NO(g) + \frac{1}{2} Br_2(g)$

This reaction is of great interest in various fields, including chemistry and environmental science. In this article, we will delve into the details of this reaction, its equilibrium constant, and the factors that affect it.

The Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a measure of the extent to which a reaction proceeds. It is defined as the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium. For the decomposition reaction of NOBr(g), the equilibrium constant (Kc) is given by:

$Kc = \frac{[NO]^1 \cdot [Br_2]^{\frac{1}{2}}}{[NOBr]}$

where [NO], [Br_2], and [NOBr] are the concentrations of NO, Br_2, and NOBr, respectively.

Calculating the Equilibrium Constant (Kc)

To calculate the equilibrium constant (Kc), we need to know the concentrations of the reactants and products at equilibrium. In this case, we are given a 0.800 mol sample of pure NOBr(g) in a rigid 1.00 L container. We can use the ideal gas law to calculate the concentration of NOBr(g) at equilibrium.

Ideal Gas Law

The ideal gas law is given by:

$PV = nRT$

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Rearranging the ideal gas law to solve for concentration, we get:

$[NOBr] = \frac{n}{V}$

Substituting the values given in the problem, we get:

$[NOBr] = \frac{0.800 \, \text{mol}}{1.00 \, \text{L}} = 0.800 \, \text{M}$

Calculating the Concentration of NO and Br_2

Since the reaction is a decomposition reaction, the concentration of NOBr(g) will decrease as the reaction proceeds. We can use the stoichiometry of the reaction to calculate the concentration of NO and Br_2.

For every mole of NOBr(g) that decomposes, one mole of NO(g) and half a mole of Br_2(g) are produced. Therefore, the concentration of NO(g) will be equal to the concentration of NOBr(g) at the start of the reaction, and the concentration of Br_2(g) will be half the concentration of NOBr(g) at the start of the reaction.

Calculating the Equilibrium Constant (Kc)

Now that we have the concentrations of the reactants and products at equilibrium, we can calculate the equilibrium constant (Kc).

$Kc = \frac{[NO]^1 \cdot [Br_2]^{\frac{1}{2}}}{[NOBr]}$

Substituting the values, we get:

$Kc = \frac{(0.800 \, \text{M})^1 \cdot (0.400 \, \text{M})^{\frac{1}{2}}}{(0.800 \, \text{M})} = 0.400$

Factors Affecting the Equilibrium Constant (Kc)

The equilibrium constant (Kc) is affected by several factors, including temperature, pressure, and the concentration of the reactants and products.

Temperature

The equilibrium constant (Kc) is temperature-dependent. As the temperature increases, the equilibrium constant (Kc) also increases. This is because higher temperatures provide more energy for the reactants to overcome the activation energy barrier and form products.

Pressure

The equilibrium constant (Kc) is also affected by pressure. As the pressure increases, the equilibrium constant (Kc) also increases. This is because higher pressures provide more opportunities for the reactants to collide and form products.

Concentration of Reactants and Products

The equilibrium constant (Kc) is also affected by the concentration of the reactants and products. As the concentration of the reactants increases, the equilibrium constant (Kc) also increases. Conversely, as the concentration of the products increases, the equilibrium constant (Kc) also increases.

Conclusion

In conclusion, the decomposition reaction of NOBr(g) is a complex process that involves the breakdown of a single compound into two simpler substances. The equilibrium constant (Kc) is a measure of the extent to which a reaction proceeds, and it is affected by several factors, including temperature, pressure, and the concentration of the reactants and products. By understanding the factors that affect the equilibrium constant (Kc), we can better predict the outcome of a reaction and design experiments to optimize the yield of the desired product.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.

Further Reading

For a more detailed discussion of the decomposition reaction of NOBr(g), see:

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.

For a more detailed discussion of the factors that affect the equilibrium constant (Kc), see:

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.
Q&A: Understanding the Decomposition Reaction of NOBr(g)

In our previous article, we discussed the decomposition reaction of NOBr(g) and its equilibrium constant (Kc). In this article, we will answer some frequently asked questions about this reaction.

Q: What is the decomposition reaction of NOBr(g)?

A: The decomposition reaction of NOBr(g) is a chemical reaction in which NOBr(g) breaks down into NO(g) and Br_2(g).

Q: What is the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: The equilibrium constant (Kc) of the decomposition reaction of NOBr(g) is 0.400.

Q: What factors affect the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: The equilibrium constant (Kc) of the decomposition reaction of NOBr(g) is affected by several factors, including temperature, pressure, and the concentration of the reactants and products.

Q: How does temperature affect the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: Temperature affects the equilibrium constant (Kc) of the decomposition reaction of NOBr(g) by providing more energy for the reactants to overcome the activation energy barrier and form products. As the temperature increases, the equilibrium constant (Kc) also increases.

Q: How does pressure affect the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: Pressure affects the equilibrium constant (Kc) of the decomposition reaction of NOBr(g) by providing more opportunities for the reactants to collide and form products. As the pressure increases, the equilibrium constant (Kc) also increases.

Q: How does the concentration of reactants and products affect the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: The concentration of reactants and products affects the equilibrium constant (Kc) of the decomposition reaction of NOBr(g) by influencing the rate of the reaction. As the concentration of the reactants increases, the equilibrium constant (Kc) also increases. Conversely, as the concentration of the products increases, the equilibrium constant (Kc) also increases.

Q: What is the significance of the equilibrium constant (Kc) of the decomposition reaction of NOBr(g)?

A: The equilibrium constant (Kc) of the decomposition reaction of NOBr(g) is significant because it provides a measure of the extent to which a reaction proceeds. By understanding the factors that affect the equilibrium constant (Kc), we can better predict the outcome of a reaction and design experiments to optimize the yield of the desired product.

Q: What are some common applications of the decomposition reaction of NOBr(g)?

A: The decomposition reaction of NOBr(g) has several common applications, including:

Production of NO(g) and Br_2(g): The decomposition reaction of NOBr(g) is used to produce NO(g) and Br_2(g) on a large scale.
Synthesis of other compounds: The decomposition reaction of NOBr(g) is used as a starting material for the synthesis of other compounds, such as NO_2(g) and BrF_3(g).
Environmental applications: The decomposition reaction of NOBr(g) is used to study the environmental fate of NOBr(g) and its impact on the atmosphere.

Q: What are some common mistakes to avoid when working with the decomposition reaction of NOBr(g)?

A: Some common mistakes to avoid when working with the decomposition reaction of NOBr(g) include:

Incorrect handling of NOBr(g): NOBr(g) is a highly reactive gas that requires careful handling to avoid accidents.
Incorrect measurement of the equilibrium constant (Kc): The equilibrium constant (Kc) of the decomposition reaction of NOBr(g) must be measured carefully to avoid errors.
Incorrect interpretation of the results: The results of the decomposition reaction of NOBr(g) must be interpreted carefully to avoid misinterpretation.

Conclusion

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.
Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.

Further Reading

For a more detailed discussion of the decomposition reaction of NOBr(g), see:

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry (10th ed.). McGraw-Hill.

For a more detailed discussion of the factors that affect the equilibrium constant (Kc), see:

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.