Passage
Household cleaners commonly contain either ammonia (NH₃) or bleach (NaOCl) as the principal active ingredient. Mixing ammonia-based and bleach-based cleaners can be hazardous, as the resulting reactions can form several toxic products. One of these reactions forms the irritant dichloramine (NHCl₂) as follows:
Reaction 1The overall reaction has a standard enthalpy change of −55 kJ/mol and a standard entropy change of −150 J/mol·K. Partial thermodynamic data for formation of Reaction 1 reagents from their elements are shown in Table 1.Table 1 Partial Data for Enthalpies, Entropies, and Free Energies of Formation of Several Compounds at 25 °C
After it is formed, dichloramine readily enters the gas phase, where it may be inhaled. In the lungs, dichloramine reacts with water to produce hydrochloric acid and ammonia, as well as reactive oxygen species. In small doses, these products cause mild irritation, but inhalation of large amounts of chloramines can lead to pneumonitis (inflammation of the lungs) and may require medical intervention.
Adapted from Trogolo D, Arey JS. Benchmark thermochemistry of chloramines, bromamines, and bromochloramines: halogen oxidants stabilized by electron correlation. Phys Chem Chem Phys. 2015;17(5) :3584-98.
-If large amounts of ammonia and bleach were mixed, emergency responders could help stop the reaction by doing which of the following?

Question

Passage
Household cleaners commonly contain either ammonia (NH₃) or bleach (NaOCl) as the principal active ingredient. Mixing ammonia-based and bleach-based cleaners can be hazardous, as the resulting reactions can form several toxic products. One of these reactions forms the irritant dichloramine (NHCl₂) as follows:

Passage Household cleaners commonly contain either ammonia (NH<sub>3</sub>) or bleach (NaOCl) as the principal active ingredient. Mixing ammonia-based and bleach-based cleaners can be hazardous, as the resulting reactions can form several toxic products. One of these reactions forms the irritant dichloramine (NHCl<sub>2</sub>) as follows: <strong>Reaction 1</strong>The overall reaction has a standard enthalpy change of −55 kJ/mol and a standard entropy change of −150 J/mol·K. Partial thermodynamic data for formation of Reaction 1 reagents from their elements are shown in Table 1.<strong>Table 1</strong> Partial Data for Enthalpies, Entropies, and Free Energies of Formation of Several Compounds at 25 °C After it is formed, dichloramine readily enters the gas phase, where it may be inhaled. In the lungs, dichloramine reacts with water to produce hydrochloric acid and ammonia, as well as reactive oxygen species. In small doses, these products cause mild irritation, but inhalation of large amounts of chloramines can lead to pneumonitis (inflammation of the lungs) and may require medical intervention. Adapted from Trogolo D, Arey JS. Benchmark thermochemistry of chloramines, bromamines, and bromochloramines: halogen oxidants stabilized by electron correlation. Phys Chem Chem Phys. 2015;17(5) :3584-98. -If large amounts of ammonia and bleach were mixed, emergency responders could help stop the reaction by doing which of the following? A) Mixing sodium hydroxide into the solution B) Adding ammonia to the solution C) Removing dichloramine from the solution D) Evaporating water from the solution

Reaction 1The overall reaction has a standard enthalpy change of −55 kJ/mol and a standard entropy change of −150 J/mol·K. Partial thermodynamic data for formation of Reaction 1 reagents from their elements are shown in Table 1.Table 1 Partial Data for Enthalpies, Entropies, and Free Energies of Formation of Several Compounds at 25 °C

After it is formed, dichloramine readily enters the gas phase, where it may be inhaled. In the lungs, dichloramine reacts with water to produce hydrochloric acid and ammonia, as well as reactive oxygen species. In small doses, these products cause mild irritation, but inhalation of large amounts of chloramines can lead to pneumonitis (inflammation of the lungs) and may require medical intervention.
Adapted from Trogolo D, Arey JS. Benchmark thermochemistry of chloramines, bromamines, and bromochloramines: halogen oxidants stabilized by electron correlation. Phys Chem Chem Phys. 2015;17(5) :3584-98.
-If large amounts of ammonia and bleach were mixed, emergency responders could help stop the reaction by doing which of the following?

Quizplus · Accepted Answer

11ecba2d_11b1_c3e3_a3bf_6b17b9836a8a_MD0008_00 A reaction's equilibrium state is the set of concentrations of products and reactants at which no new products or reactants are formed. Under equilibrium conditions, the ratio of product concentrations to reactant concentrations equals the equilibrium constant for the reaction, K_eq. Note that this is not necessarily the same as when product concentration equals reactant concentration, in which case K_eq would equal 1. Le Châtelier's principle states that any change to a system that moves it away from equilibrium, such as the addition of products or reactants, will cause it to adjust accordingly to come back to equilibrium. Therefore, the addition of reactants to the system will drive the formation of more products, and the addition of products will drive the formation of reactants. Similarly, the removal of reactants drives the system toward reactant formation, and the removal of products drives the system toward product formation. Sodium hydroxide (NaOH) is one of the products of the reaction described in the passage. Therefore, the addition of NaOH will drive the reaction toward reactant formation and away from product formation, which will help stop the reaction from continuing. (Choice B) Ammonia is one of the reactants. Adding it to the solution will drive the formation of more products. (Choice C) Dichloramine is one of the products of the reaction, and its removal from the system will drive further product formation. During the reaction, dichloramine naturally leaves the solution and enters the gas phase, and the reaction is induced to form more dichloramine. (Choice D) Evaporating water from the reaction would concentrate its components and most likely result in more rapid product formation. On the other hand, diluting the reaction would help slow it. Educational objective: Le Châtelier's principle states that changes to a system that move it away from equilibrium will cause the system to adjust and come back to equilibrium. The addition of reactants or removal of products results in product formation, and the addition of products or removal of reactants results in reactant formation.

Passage Household Cleaners Commonly Contain Either Ammonia (NH3) or Bleach (NaOCl)

Passage Household Cleaners Commonly Contain Either Ammonia (NH₃) or Bleach (NaOCl)