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Chapter 6: Problem 46

The reaction $$ \mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q) $$ is the last step in the commercial production of sulfuric acid. The enthalpy change for this reaction is \(-227 \mathrm{kJ} .\) In designing a sulfuric acid plant, is it necessary to provide for heating or cooling of the reaction mixture? Explain.

Short Answer

Expert verified
In designing a sulfuric acid plant, there is no specific need to provide heating or cooling for the reaction mixture, as the reaction is exothermic, releasing heat to the surroundings and providing the necessary heat for the entire process. However, it is essential to consider safety guidelines and regulations to ensure that the generated heat doesn't pose any risks to equipment or personnel.

Step by step solution

01

Determine the temperature requirement of the reaction

The given reaction is the last step in the commercial production of sulfuric acid. We are not given any specific temperature requirement for the reaction to proceed. However, we will analyze the reaction based on the enthalpy change provided.
02

Analyze the enthalpy change value

The enthalpy change for the given reaction is -227 kJ. This negative value indicates that the reaction releases energy in the form of heat to the surroundings, and this type of reaction is considered exothermic.
03

Determine the necessity of heating or cooling

Because the reaction releases heat to the surroundings, and we are not given any particular temperature requirements for the reaction, we can assume that it doesn't require any additional source of heat or external cooling system unless there's a safety issue related to high operating temperatures. The reaction itself should provide the necessary heat for the entire process. Hence, there is no need to provide for specific heating or cooling of the reaction mixture in the sulfuric acid plant, but it is important to consider safety guidelines and regulations to ensure that the generated heat doesn't pose any risks to equipment or personnel.

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Most popular questions from this chapter

It has been determined that the body can generate 5500 \(\mathrm{kJ}\) of energy during one hour of strenuous exercise. Perspiration is the body's mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is 40.6 \(\mathrm{kJ} / \mathrm{mol.} )\)

If a student performs an endothermic reaction in a calorimeter, how does the calculated value of \(\Delta H\) differ from the actual value if the heat exchanged with the calorimeter is not taken into account?

Consider 2.00 moles of an ideal gas that are taken from state \(A\) \(\left(P_{A}=2.00 \mathrm{atm}, V_{A}=10.0 \mathrm{L}\right)\) to state \(B\left(P_{B}=1.00 \mathrm{atm}, V_{B}=\right.\) 30.0 \(\mathrm{L}\) ) by two different pathways: These pathways are summarized on the following graph of \(P\) versus \(V :\) Calculate the work (in units of \(\mathrm{J} )\) associated with the two path- ways. Is work a state function? Explain.

The standard enthalpy of formation of \(\mathrm{H}_{2} \mathrm{O}(l)\) at 298 \(\mathrm{K}\) is \(-285.8 \mathrm{kJ} / \mathrm{mol}\) . Calculate the change in internal energy for the following process at 298 \(\mathrm{K}\) and \(1 \mathrm{atm} :\) $$ \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \quad \Delta E^{\circ}=? $$ (Hint: Using the ideal gas equation, derive an expression for work in terms of \(n, R,\) and \(T\) )

If the internal energy of a thermodynamic system is increased by $300 . \mathrm{J}\( while 75 \)\mathrm{J}$ of expansion work is done, how much heat was transferred and in which direction, to or from the system?
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