Thermal equilibrium (thermodynamics)

[YuUZoe]

consider a system composed of a mixture of 2.5 kg of ice and 50 gr of liquid water and a small separate container of finely powdered salt. this physical system is contained in a fully insulated container that prevents all thermal interactions with the environment. both the salt and the ice-water mixture are initially at the freezing point, 0 degree celcius. the salt is then added to the ice-water mixture, and the system of ice-water and salt is allowed to come to thermal equilibrium. the final equilibrium temperature is less than 0 degree C. use the energy interaction model to predict if there will be a greater or lesser amount of ice in the final equilibrium state than in the initial state before the salt was added.

~how do you solve this?I'm really confused. Please solve this question step-by-step.

Thank you

 

[Andrew Mason]

consider a system composed of a mixture of 2.5 kg of ice and 50 gr of liquid water and a small separate container of finely powdered salt. this physical system is contained in a fully insulated container that prevents all thermal interactions with the environment. both the salt and the ice-water mixture are initially at the freezing point, 0 degree celcius. the salt is then added to the ice-water mixture, and the system of ice-water and salt is allowed to come to thermal equilibrium. the final equilibrium temperature is less than 0 degree C. use the energy interaction model to predict if there will be a greater or lesser amount of ice in the final equilibrium state than in the initial state before the salt was added.

~how do you solve this?I'm really confused. Please solve this question step-by-step.

Thank you

The ice melting represents an increase in energy by the mass of the ice x the heat of fusion/unit mass. The total energy, however, does not change. In order to provide this heat, the salt water must cool down. How much must it cool down by?

AM

 

[baba89]

for your question. I am happy to provide a step-by-step explanation of how to solve this problem using the energy interaction model.

Step 1: Understand the Problem
The first step in solving any problem is to understand the given information and what is being asked. In this case, we are dealing with a physical system composed of ice, liquid water, and salt. The system is fully insulated, meaning there are no thermal interactions with the environment. The initial state of the system is at the freezing point, and the salt is added to the mixture. We are asked to predict if there will be a greater or lesser amount of ice in the final equilibrium state compared to the initial state.

Step 2: Identify Relevant Concepts
In order to solve this problem, we need to apply the energy interaction model, which is a fundamental concept in thermodynamics. This model states that energy cannot be created or destroyed, but it can be transferred or transformed from one form to another. In this case, we are dealing with thermal energy, which is the energy associated with the temperature of a system.

Step 3: Apply the Energy Interaction Model
In the initial state, we have a mixture of ice and liquid water at the freezing point. This means that the ice is at 0 degrees Celsius and the liquid water is also at 0 degrees Celsius. When the salt is added to the mixture, it will start to dissolve and release ions into the water. This process is called dissolving and it requires energy, which is taken from the surrounding environment. As a result, the temperature of the mixture will decrease.

Step 4: Understand the Effect of Salt on Freezing Point
One important concept to understand in this problem is the effect of salt on the freezing point of water. When salt is added to water, it lowers the freezing point of the water. This is because the salt ions disrupt the formation of ice crystals, making it more difficult for water to freeze. As a result, the freezing point of the mixture will be lower than 0 degrees Celsius.

Step 5: Predict the Final Equilibrium State
Based on the energy interaction model and the effect of salt on the freezing point of water, we can predict that there will be a greater amount of ice in the final equilibrium state compared to the initial state. This is because the addition of salt lowers the freezing point of the water, making it more difficult for the water to freeze. As a result, there will