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Chapter 13: Problem 10

In Section 13.1 of your text, it is mentioned that equilibrium is reached in a "closed system." What is meant by the term "closed system," and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.

Short Answer

Expert verified
A closed system is one where there is no exchange of matter with its surroundings but allows the exchange of energy. Equilibrium is reached in a closed system because the constant mass allows the system to reach a state of balance between processes occurring within it, maintaining constant properties like temperature, pressure, and concentration. On the other hand, an open system allows exchanges of both matter and energy with its surroundings. Equilibrium is not reached in an open system because the continuous exchange of matter causes ongoing changes in the system's properties, making it impossible to achieve a stable state of balance.

Step by step solution

01

Define Closed System

A closed system is a physical system that does not allow the exchange of matter with its surroundings but allows the exchange of energy. This means that the total mass in the system remains constant, but heat and work can be transferred between the system and its surroundings.
02

Define Open System

An open system, on the other hand, is one that can exchange both matter and energy with its surroundings. In an open system, there are no barriers to mass flow, so substances can freely enter or exit the system.
03

Explain the Necessity of a Closed System for Equilibrium

Equilibrium is reached when the rate of change in a system becomes zero, and the system is said to be at a state of balance. In a closed system, the total mass of the system remains constant, allowing the system to reach a state of balance between the processes occurring within it, and maintaining constant temperature, pressure, and concentration. If a system is not closed, the constant transfer of matter would cause a continuous change in the properties of the system, making it impossible to reach equilibrium.
04

Explain why Equilibrium is Not Reached in an Open System

In an open system, matter can continuously enter and leave the system, causing changes in the properties (such as concentration, pressure, and temperature) of the system. This continuous exchange of matter prevents the system from reaching a state of balance, as the processes within the system are constantly affected by the addition or removal of substances. Consequently, equilibrium cannot be achieved in an open system due to the ongoing changes and lack of stability.

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Most popular questions from this chapter

Le Chatelier's principle is stated (Section 13.7\()\) as follows: "If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change." The system $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$ is used as an example in which the addition of nitrogen gas at equilibrium results in a decrease in \(\mathrm{H}_{2}\) concentration and an increase in \(\mathrm{NH}_{3}\) concentration. In the experiment the volume is assumed to be constant. On the other hand, if \(\mathrm{N}_{2}\) is added to the reaction system in a container with a piston so that the pressure can be held constant, the amount of \(\mathrm{NH}_{3}\) actually could decrease and the concentration of \(\mathrm{H}_{2}\) would increase as equilibrium is reestablished. Explain how this can happen. Also, if you consider this same system at equilibrium, the addition of an inert gas, holding the pressure constant, does affect the equilibrium position. Explain why the addition of an inert gas to this system in a rigid container does not affect the equilibrium position.

The equilibrium constant \(K_{\mathrm{p}}\) is \(2.4 \times 10^{3}\) at a certain temperature for the reaction $$2 \mathrm{NO}(g) \leftrightharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g)$$ For which of the following sets of conditions is the system at equilibrium? For those not at equilibrium, in which direction will the system shift? a. $P_{\mathrm{NO}}=0.012 \mathrm{atm}, P_{\mathrm{N}_{2}}=0.11 \mathrm{atm}, P_{\mathrm{O}_{2}}=2.0 \mathrm{atm}$ b. $P_{\mathrm{NO}}=0.0078 \mathrm{atm}, P_{\mathrm{N}_{2}}=0.36 \mathrm{atm}, P_{\mathrm{O}_{2}}=0.67 \mathrm{atm}$ c. $P_{\mathrm{NO}}=0.0062 \mathrm{atm}, P_{\mathrm{N}_{2}}=0.51 \mathrm{atm}, P_{\mathrm{O}_{2}}=0.18 \mathrm{atm}$

Consider the following reaction at \(725^{\circ} \mathrm{C} :\) $$\mathrm{C}(s)+\mathrm{CO}_{2}(g) \leftrightharpoons 2 \mathrm{CO}(g)$$ At equilibrium, a \(4.50-\mathrm{L}\) container has 2.6 \(\mathrm{g}\) of carbon, \(\mathrm{CO}_{2}\) at a partial pressure of \(0.0020 \mathrm{atm},\) and a total pressure of 0.572 atm. Calculate \(K_{\mathrm{p}}\) for this reaction at \(725^{\circ} \mathrm{C}\)

For the reaction $$\mathrm{C}(s)+\mathrm{CO}_{2}(g) \leftrightharpoons 2 \mathrm{CO}(g)$$ \(K_{\mathrm{p}}=2.00\) at some temperature. If this reaction at equilibrium has a total pressure of 6.00 \(\mathrm{atm}\) , determine the partial pressures of \(\mathrm{CO}_{2}\) and \(\mathrm{CO}\) in the reaction container.

Old-fashioned "smelling salts" consist of ammonium carbonate, (NH $_{4} )_{2} \mathrm{CO}_{3}$ . The reaction for the decomposition of ammonium carbonate $$\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(s) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$ is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
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