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Chapter 6: Problem 8

Stoichiometry is based on the law of conservation of mass. On what law is thermochemistry based?

Short Answer

Expert verified
The first law of thermodynamics (or the law of energy conservation) is the law on which thermochemistry is based.

Step by step solution

01

Understanding Thermochemistry

Thermochemistry is a branch of chemistry concerning the study of heat in relation to chemical reactions. It mainly focuses on how heat transfers during chemical reactions and how energy changes from one form to another.
02

Identify the Law

The main law that governs thermochemistry is the 'First Law of Thermodynamics'. This law, also known as law of energy conservation, states that energy can be neither created nor destroyed but only transformed from one form to another.

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Most popular questions from this chapter

Ice at \(0^{\circ} \mathrm{C}\) is placed in a Styrofoam cup containing \(361 \mathrm{~g}\) of a soft drink at \(23^{\circ} \mathrm{C}\). The specific heat of the drink is about the same as that of water. Some ice remains after the ice and soft drink reach an equilibrium temperature of \(0^{\circ} \mathrm{C}\). Determine the mass of ice that has melted. Ignore the heat capacity of the cup. (Hint: It takes 334 J to melt \(1 \mathrm{~g}\) of ice at \(\left.0^{\circ} \mathrm{C} .\right)\)

Determine the amount of heat (in \(\mathrm{kJ}\) ) given off when \(1.26 \times 10^{4} \mathrm{~g}\) of ammonia are produced according to the equation $$ \begin{aligned} \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow & 2 \mathrm{NH}_{3}(g) \\\ \Delta H_{\mathrm{rxn}}^{\circ} &=-92.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Assume that the reaction takes place under standardstate conditions at \(25^{\circ} \mathrm{C}\).

Define calorimetry and describe two commonly used calorimeters. In a calorimetric measurement, why is it important that we know the heat capacity of the calorimeter? How is this value determined?

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.

How are the standard enthalpies of formation of an element and of a compound determined?
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