You may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts with ammonia to produce toxic chloramines, such as NH2Cl. For example, in basic solution: OCl-1aq2 + NH31aq2S OH-1aq2 + NH2Cl1aq2 (a) The following initial rate data for this reaction were obtained in basic solution at 25 °C What is the rate law for the reaction? What is the numerical value of the rate constant k, including the correct units?

Verified step by step guidance

1

insert step 1: Identify the general form of the rate law for the reaction. The rate law is typically expressed as: rate = k [OCl^-]^m [NH3]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to OCl^- and NH3, respectively.

insert step 2: Use the initial rate data provided in the table to determine the reaction orders m and n. This involves comparing the rates of reaction when the concentration of one reactant is changed while the other is held constant.

View full solution

insert step 3: Calculate the order of the reaction with respect to OCl^- by comparing experiments where the concentration of NH3 is constant. Use the formula: (rate1/rate2) = ([OCl^-]_1/[OCl^-]_2)^m.

insert step 4: Calculate the order of the reaction with respect to NH3 by comparing experiments where the concentration of OCl^- is constant. Use the formula: (rate1/rate2) = ([NH3]_1/[NH3]_2)^n.

insert step 5: Once the orders m and n are determined, use any set of experimental data to solve for the rate constant k. Substitute the known values of rate, [OCl^-], and [NH3] into the rate law and solve for k, ensuring the units are consistent.

Verified Solution

Video duration:

10m

Play a video:

This video solution was recommended by our tutors as helpful for the problem above.

0

Was this helpful?

0

Bookmarked

Key Concepts

Rate Law

The rate law of a chemical reaction expresses the relationship between the reaction rate and the concentration of reactants. It is typically formulated as rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B. Understanding the rate law is crucial for predicting how changes in concentration affect the speed of the reaction.

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a particular temperature. It reflects the intrinsic speed of the reaction and is influenced by factors such as temperature and the presence of catalysts. The units of k vary depending on the overall order of the reaction, making it essential to determine the correct units when calculating k.

Reaction Order

The reaction order is the sum of the exponents in the rate law and indicates how the rate of reaction depends on the concentration of reactants. It can be determined experimentally and can be zero, first, second, or higher. Knowing the reaction order helps in understanding the mechanism of the reaction and how different concentrations will affect the rate.

Previous problemNext problem

Related Practice

Textbook Question

For the thermal decomposition of nitrous oxide, 2 N2O1g2S 2 N21g2 + O21g2, values of the parameters in the Arrhenius equation are A = 4.2 * 109 s-1 and Ea = 222 kJ>mol. If a stream of N2O is passed through a tube 25 mm in diameter and 20 cm long at a flow rate of 0.75 L/min at what temperature should the tube be maintained to have a partial pressure of 1.0 mm of O2 in the exit gas? Assume that the total pressure of the gas in the tube is 1.50 atm.

866

views

Textbook Question

A 0.500 L reaction vessel equipped with a movable piston is filled completely with a 3.00% aqueous solution of hydrogen peroxide. The H2O2 decomposes to water and O2 gas in a first-order reaction that has a half-life of 10.7 h. As the reaction proceeds, the gas formed pushes the piston against a constant external atmospheric pressure of 738 mm Hg. Calculate the PV work done (in joules) after a reaction time of 4.02 h. (You may assume that the density of the solution is 1.00 g/mL and that the temperature of the system is maintained at 20 °C.)

626

views

Open Question

At 791 K and relatively low pressures, the gas-phase decomposition of acetaldehyde (CH3CHO) is second order in acetaldehyde. CH3CHO(g) → CH4(g) + CO(g) The total pressure of a particular reaction mixture was found to vary as follows:

(a) Use the pressure data to determine the value of the rate constant in units of atm⁻¹ s⁻¹. (b) What is the rate constant in the usual units of M⁻¹ s⁻¹?

Download the Mobile app

Terms of use

Privacy

Cookies

Do not sell my personal information

Accessibility

Patent notice

Sitemap

© 1996–2025 Pearson All rights reserved.

Verified step by step guidance

1. insert step 1: Identify the general form of the rate law for the reaction. The rate law is typically expressed as: rate = k [OCl^-]^m [NH3]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to OCl^- and NH3, respectively.
2. insert step 2: Use the initial rate data provided in the table to determine the reaction orders m and n. This involves comparing the rates of reaction when the concentration of one reactant is changed while the other is held constant.
3. insert step 3: Calculate the order of the reaction with respect to OCl^- by comparing experiments where the concentration of NH3 is constant. Use the formula: (rate1/rate2) = ([OCl^-]_1/[OCl^-]_2)^m.
4. insert step 4: Calculate the order of the reaction with respect to NH3 by comparing experiments where the concentration of OCl^- is constant. Use the formula: (rate1/rate2) = ([NH3]_1/[NH3]_2)^n.
5. insert step 5: Once the orders m and n are determined, use any set of experimental data to solve for the rate constant k. Substitute the known values of rate, [OCl^-], and [NH3] into the rate law and solve for k, ensuring the units are consistent.

Key Concepts

Rate Law

The rate law of a chemical reaction expresses the relationship between the reaction rate and the concentration of reactants. It is typically formulated as rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B. Understanding the rate law is crucial for predicting how changes in concentration affect the speed of the reaction.

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a particular temperature. It reflects the intrinsic speed of the reaction and is influenced by factors such as temperature and the presence of catalysts. The units of k vary depending on the overall order of the reaction, making it essential to determine the correct units when calculating k.

Reaction Order

The reaction order is the sum of the exponents in the rate law and indicates how the rate of reaction depends on the concentration of reactants. It can be determined experimentally and can be zero, first, second, or higher. Knowing the reaction order helps in understanding the mechanism of the reaction and how different concentrations will affect the rate.