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Chapter 6: Problem 53

Nitric acid, a source of many nitrogen compounds, is produced from nitrogen dioxide. An old process for making nitrogen dioxide employed nitrogen and oxygen. $$ \mathrm{N}_{2}(g)+2 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) $$ The reaction absorbs \(66.2 \mathrm{~kJ}\) of heat per \(2 \mathrm{~mol} \mathrm{NO}_{2}\) produced. Is the reaction endothermic or exothermic? What is the value of \(q\) ?

Short Answer

Expert verified
The reaction is endothermic; \(q = +66.2\, \mathrm{kJ}\).

Step by step solution

01

Understanding the Reaction

The reaction given is: \( \mathrm{N}_{2}(g) + 2 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}_{2}(g) \). This is a chemical reaction involving nitrogen and oxygen to form nitrogen dioxide. The problem states that the reaction absorbs \(66.2\, \mathrm{kJ}\) of heat per \(2\, \mathrm{mol}\) of \(\mathrm{NO}_{2}\) produced.
02

Identifying Reaction Type

A reaction is considered endothermic if it absorbs heat from the surroundings, which is indicated by a positive value for heat (q). Since the problem states the reaction absorbs \(66.2\, \mathrm{kJ}\), this signifies that it is an endothermic reaction.
03

Finding the Value of \(q\)

In thermodynamics, \(q\) represents the heat absorbed or released during a reaction. For an endothermic reaction, \(q\) is positive. Here, since \(66.2\, \mathrm{kJ}\) is absorbed, it means \(q = +66.2\, \mathrm{kJ}\) for \(2\, \mathrm{mol}\) of \(\mathrm{NO}_{2}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Thermodynamics
Chemical thermodynamics is the study of the interrelation of heat with chemical reactions. It helps us understand how energy is transferred within chemical processes. In any chemical reaction, energy can be absorbed or released, and chemical thermodynamics provides the tools to determine these energy changes.

There are two main types of reactions in thermodynamics: endothermic and exothermic.
  • Endothermic reactions absorb heat, meaning energy is taken in from the surroundings. This results in a positive heat change ( q ) since the system gains energy.
  • Exothermic reactions release heat, indicating energy is expelled to the surroundings. This results in a negative heat change ( q ) since the system loses energy.
When dealing with chemical reactions, understanding whether a reaction is endothermic or exothermic is crucial for predicting reaction behavior and feasibility.
Reaction Heat
Reaction heat, represented by q , is the amount of heat absorbed or released during a chemical reaction. This value is essential for determining the nature of the reaction and the energy dynamics involved.

When a reaction absorbs heat, such as in the case of the formation of nitrogen dioxide ( NO_2 ), it indicates an endothermic reaction. Here, the system requires heat from the surroundings to proceed. The given reaction of N_2 and O_2 forming NO_2 involves the absorption of 66.2 kJ of heat per 2 mol of NO_2 produced, resulting in a positive q value.
  • Positive q : Heat is absorbed, the system gains energy.
  • Negative q : Heat is released, energy exits the system.
This distinction helps in predicting temperature changes during the reaction and assessing associated energy requirements.
Nitric Acid Production
Nitric acid production involves a series of chemical reactions, starting with nitrogen dioxide ( NO_2 ) as a key reactant. Nitrogen dioxide is formed from nitrogen ( N_2 ) and oxygen ( O_2 ), as shown in the provided equation. This reaction is crucial in the industrial preparation of nitric acid, a compound with numerous industrial applications, including fertilizers and explosives.

The production process typically involves oxidizing nitrogen in the air to form nitrogen monoxide, which is further oxidized to nitrogen dioxide. Following oxidation, nitrogen dioxide reacts with water, yielding nitric acid ( HNO_3 ).
  • Stage 1: Formation of NO_2 from N_2 and O_2 is endothermic, requiring heat.
  • Stage 2: Subsequent reactions involve NO_2 reacting with water to eventually form nitric acid.
Understanding these steps is vital as each stage has specific energy requirements and environmental considerations essential for efficiently producing nitric acid on an industrial scale.

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Most popular questions from this chapter

A piece of iron was heated to \(95.4^{\circ} \mathrm{C}\) and dropped into a constant-pressure calorimeter containing \(284 \mathrm{~g}\) of water at \(32.2^{\circ} \mathrm{C}\). The final temperature of the water and iron was \(51.9^{\circ} \mathrm{C}\). Assuming that the calorimeter itself absorbs a negligible amount of heat, what was the mass (in grams) of the piece of iron? The specific heat of iron is \(0.449 \mathrm{~J} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\), and the specific heat of water is \(4.18 \mathrm{~J} /\) \(\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)\)

List some rocket fuels and corresponding oxidizers. Give thermochemical equations for the exothermic reactions of these fuels with the oxidizers.

Any object, be it a space satellite or a molecule, must attain an initial upward velocity of at least \(11.2 \mathrm{~km} / \mathrm{s}\) in order to escape the gravitational attraction of the earth. What would be the kinetic energy in joules of a satellite weighing \(2458 \mathrm{lb}\) that has the speed equal to this escape velocity of \(11.2 \mathrm{~km} / \mathrm{s} ?\)

Dry ice is solid carbon dioxide; it vaporizes at room temperature and normal pressures to the gas. Suppose you put \(21.5 \mathrm{~g}\) of dry ice in a vessel fitted with a piston (similar to the one in Figure 6.9 but with the weight replaced by the atmosphere), and it vaporizes completely to the gas, pushing the piston upward until its pressure and temperature equal those of the surrounding atmosphere at \(24.0^{\circ} \mathrm{C}\) and \(751 \mathrm{mmHg}\). Calculate the work done by the gas in expanding against the atmosphere. Neglect the volume of the solid carbon dioxide, which is very small in comparison to the volume of the gas phase.

What is meant by the reference form of an element? What is the standard enthalpy of formation of an element in its reference form?
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