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Chapter 5: Problem 22

In a thermodynamic study, a scientist focuses on the properties of a solution in an apparatus as illustrated. A solution is continuously flowing into the apparatus at the top and out at the bottom, such that the amount of solution in the apparatus is constant with time. (a) Is the solution in the apparatus a closed system, open system, or isolated system? (b) If the inlet and outlet were closed, what type of system would it be?

Short Answer

Expert verified
(a) the solution in the apparatus is an open system. (b) with the inlet and outlet closed, it would be a closed system.

Step by step solution

01

Case (a): With the solution continuously flowing in and out.

In this case, the solution in the apparatus has both mass and energy exchange with its surroundings as it is continuously flowing into the apparatus at the top and out at the bottom. As there is mass and energy exchange with the surroundings, this makes it an open system. So, the solution in the apparatus is an open system.
02

Case (b): With the inlet and outlet closed.

When the inlet and outlet are closed, there is no mass exchange between the solution in the apparatus and the surroundings. However, in this case, there can still be energy exchange between the system and its surroundings (e.g., due to heat transfer). Since there is only energy exchange and no mass exchange, this makes it a closed system. So, with the inlet and outlet closed, it would be a closed system.

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Most popular questions from this chapter

Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing \(1000 \mathrm{~g}\) of water at \(10.0^{\circ} \mathrm{C}\). Object A increases the water temperature by $3.50^{\circ} \mathrm{C} ; \mathrm{B}\( increases the water temperature by \)2.60{ }^{\circ} \mathrm{C}$. (a) Which object has the larger heat capacity? (b) What can you say about the specific heats of \(\mathrm{A}\) and \(\mathrm{B}\) ?

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Without doing any calculations, predict the sign of \(\Delta H\) for each of the following reactions: (a) $\mathrm{NaCl}(s) \longrightarrow \mathrm{Na}^{+}(g)+\mathrm{Cl}^{-}(\mathrm{g})$ (b) \(2 \mathrm{H}(g) \longrightarrow \mathrm{H}_{2}(g)\) (c) \(\mathrm{Na}(g) \longrightarrow \mathrm{Na}^{+}(g)+\mathrm{e}^{-}\) (d) \(\mathrm{I}_{2}(s) \longrightarrow \mathrm{I}_{2}(l)\)

(a) Write an equation that expresses the first law of thermodynamics in terms of heat and work. (b) Under what conditions will the quantities \(q\) and \(w\) be negative numbers?

A coffee-cup calorimeter of the type shown in Figure 5.18 contains $150.0 \mathrm{~g}\( of water at \)25.2^{\circ} \mathrm{C}\(. A \)200-\mathrm{g}$ block of silver metal is heated to \(100.5^{\circ} \mathrm{C}\) by putting it in a beaker of boiling water. The specific heat of \(\mathrm{Ag}(s)\) is $0.233 \mathrm{~J} /(\mathrm{g} \cdot \mathrm{K})\(. The \)\mathrm{Ag}$ is added to the calorimeter, and after some time the contents of the cup reach a constant temperature of \(30.2^{\circ} \mathrm{C} .(\mathbf{a})\) Determine the amount of heat, in J, lost by the silver block. (b) Determine the amount of heat gained by the water. The specific heat of water is $4.184 \mathrm{~J} /(\mathrm{g} \cdot \mathrm{K}) .(\mathbf{c})$ The difference between your answers for (a) and (b) is due to heat loss through the Styrofoam \(^{\circ}\) cups and the heat necessary to raise the temperature of the inner wall of the apparatus. The heat capacity of the calorimeter is the amount of heat necessary to raise the temperature of the apparatus (the cups and the stopper) by \(1 \mathrm{~K} .\) Calculate the heat capacity of the calorimeter in \(\mathrm{J} / \mathrm{K}\). (d) What would be the final temperature of the system if all the heat lost by the silver block were absorbed by the water in the calorimeter?
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