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Chapter 6: Problem 41

What is meant by the standard enthalpy of a reaction?

Short Answer

Expert verified
The standard enthalpy of a reaction, \( \Delta H^0 \), refers to the change in enthalpy (total energy) that comes with a reaction taking place under standard conditions. These conditions usually are 25掳C (298 K), 1 bar or 1 atm pressure, and concentrations of 1 mol/L for all substances in solution.

Step by step solution

01

Define Enthalpy

The term 'enthalpy' refers to the total energy of a thermodynamic system. It includes the internal energy of the system as well as the energy involved in doing work against the system's surrounding atmosphere.
02

Introduce Concept of Standard Enthalpy

The 'standard' in standard enthalpy refers to 'Standard conditions', usually defined as 25掳C (298 K), 1 bar or 1 atm pressure, and solutions at 1 mol/L. Standard states are important for calculating or comparing thermodynamic quantities consistently.
03

Explain Standard Enthalpy of a Reaction

The standard enthalpy of a reaction (\( \Delta H^0 \)) is the change in enthalpy that comes along with a chemical reaction happening at standard conditions. In other words, it is the heat absorbed or released in a reaction under standard conditions.

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Most popular questions from this chapter

I he enthaipy of combustion benzo1c acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be \(-3226.7 \mathrm{~kJ} / \mathrm{mol}\). When \(1.9862 \mathrm{~g}\) of benzoic acid are burned in a calorimeter, the temperature rises from \(21.84^{\circ} \mathrm{C}\) to \(25.67^{\circ} \mathrm{C}\). What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly \(2000 \mathrm{~g} .)\)

Explain the meaning of this thermochemical equation: $$ \begin{aligned} 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g) &+6 \mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H=&-904 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$

Producer gas (carbon monoxide) is prepared by passing air over red-hot coke: $$ \mathrm{C}(s)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}(g) $$ Water gas (mixture of carbon monoxide and hydrogen) is prepared by passing steam over red-hot coke: $$ \mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g) $$ For many years, both producer gas and water gas were used as fuels in industry and for domestic cooking. The large-scale preparation of these gases was carried out alternately, that is, first producer gas, then water gas, and so on. Using thermochemical reasoning, explain why this procedure was chosen.

A gas expands and does \(P-V\) work on the surroundings equal to \(325 \mathrm{~J}\). At the same time, it absorbs \(127 \mathrm{~J}\) of heat from the surroundings. Calculate the change in energy of the gas.

The standard enthalpy change \(\Delta H^{\circ}\) for the thermal decomposition of silver nitrate according to the following equation is \(+78.67 \mathrm{~kJ}\) : $$ \mathrm{AgNO}_{3}(s) \longrightarrow \mathrm{AgNO}_{2}(s)+\frac{1}{2} \mathrm{O}_{2}(g) $$ The standard enthalpy of formation of \(\mathrm{AgNO}_{3}(s)\) is \(-123.02 \mathrm{~kJ} / \mathrm{mol}\). Calculate the standard enthalpy of formation of \(\mathrm{AgNO}_{2}(s)\).
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