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Chapter 6: Problem 42

Write the equation for calculating the enthalpy of a reaction. Define all the terms.

Short Answer

Expert verified
The enthalpy of a reaction is calculated using the equation \(\Delta H = \Delta E + P \Delta V\), where \(\Delta H\) is the change in enthalpy, \(\Delta E\) is the change in internal energy of the system, \(P\) is the pressure of the system, and \(\Delta V\) is the change in volume of the system.

Step by step solution

01

Writing the Equation

The equation for calculating the enthalpy of a reaction is given by \[ \Delta H = \Delta E + P \Delta V \] where \(\Delta H\) is the change in enthalpy, \(\Delta E\) is the change in internal energy, \(P\) is the pressure of the system, and \(\Delta V\) is the change in volume of the system.
02

Defining The Terms

1. \(\Delta H\) is the change in enthalpy. It indicates the amount of energy absorbed or released during a reaction. \n2. \(\Delta E\) is the change in internal energy. This is the energy needed to create the reaction, excluding the work done by the reaction. \n3. \(P\) represents the pressure of the system. In chemistry, this is typically in atmospheres (atm). \n4. \(\Delta V\) is the change in volume. This represents the difference in volume between the reactants and the products.

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Most popular questions from this chapter

Consider the reaction $$ \begin{aligned} \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow & 2 \mathrm{NH}_{3}(g) \\\ \Delta H_{\mathrm{rxn}}^{\circ} &=-92.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ If 2.0 moles of \(\mathrm{N}_{2}\) react with 6.0 moles of \(\mathrm{H}_{2}\) to form \(\mathrm{NH}_{3},\) calculate the work done (in joules) against a pressure of 1.0 atm at \(25^{\circ} \mathrm{C}\). What is \(\Delta E\) for this reaction? Assume the reaction goes to completion.

A piece of silver of mass \(362 \mathrm{~g}\) has a heat capacity of \(85.7 \mathrm{~J} /{ }^{\circ} \mathrm{C}\). What is the specific heat of silver?

Why are cold, damp air and hot, humid air more uncomfortable than dry air at the same temperatures? (The specific heats of water vapor and air are approximately \(1.9 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\) and \(1.0 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\), respectively.

Determine the amount of heat (in kJ) given off when \(1.26 \times 10^{4} \mathrm{~g}\) of \(\mathrm{NO}_{2}\) are produced according to the equation $$ \begin{aligned} 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow & 2 \mathrm{NO}_{2}(g) \\ \Delta H &=-114.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$

Decomposition reactions are usually endothermic, whereas combination reactions are usually exothermic. Give a qualitative explanation for these trends.
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