A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a...

A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a
10.00 g sample of iron (specific heat capacity = 0.45 J °C-1 g-1) are heated to
100.0 °C. The mixture of hot iron and aluminum is then dropped into 91.9 g of
water at 23.7 °C.
i) State the conditions for phase equilibrium of this system.

NOTE: For an isolated system, the equilibrium state corresponds to the state with maximum entropy.

Solutions

Expert Solution

Hi Dear Respected student I'm glad to answer such a nice question for you. I hope it helps. I tried my best to provide you with a quality answer with you . I tried to utilize my full time and knowledge for this. Its quite easy and simple I believe that you will understand this in one read. Yes you can do this. Please carefully go through answer till last word. And oh yes I appreciate your hunger of grabbing knowledge keep it always up like this.

So here is your answer :

Please Feel free to ask you doubts if any. Your suggestions are most welcomed. To improve our work quality.
Please appreciate my hardwork by upvote/thumbs it will be really helpful .
Thanks for your valuable time.
Thanks for choosing this platform. All the best for your future and career. Keep learning like this always. Stay safe stay healthy. Take a good care of yourself and family . Have a great life ahead

Thanks you so much:)

genius_generous answered 1 year ago

Next > < Previous

Related Solutions

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as...

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as 4.184 J/(g*C) for this problem. For water, DHfus = 6.001 kJ/mol at 0 C. a. A 10.0 gram ice cube at -10.0 C is placed into 45.0 mL of water at 40 C. Determine the final physical state and temperature of the result. Calculate DS for the ice cube and the surrounding water, and Use the value DStot to explain why this process is...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained when 20 q of water is heated from 22˚C to 77˚C? 2. What is the heat in J to melt 100g of NaCl when the HF for NaCl is 518 J/g? 3. What is the heat in J to equate 50 g Acetic Acid when the HE = 390 J/g?

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 20.4 g of steam at 162°C is condensed, cooled, and frozen to ice at -50.°C.

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 13.2 g of steam at 192°C is condensed, cooled, and frozen to ice at -50.°C.

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 27.1 g of steam at 216°C is condensed, cooled, and frozen to ice at -50.°C. ______KJ Please show the steps

a) A 500.-g iceberg at -5.00°C is placed in a 226 g beaker with specific heat...

a) A 500.-g iceberg at -5.00°C is placed in a 226 g beaker with specific heat capacity 840 J/kg °C at temperature 15.0°C that contains 220 g of water. What is the minimum amount of steam needed to add into the system in order to melt the iceberg?

In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is...

In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is mixed with 60 g of water at 20 Celsius, with the mixture thermally isolated. You will need to look up the specific heat of water. (a) What is the equilibrium temperature? (b) What is the entropy change for the aluminum block? (c) What is the entropy change for the water? (d) What is the entropy change for the aluminum-water system?

A 62.5 g of iron with a heat capacity of .450 J/C is heated to 100...

A 62.5 g of iron with a heat capacity of .450 J/C is heated to 100 degree C. It is then transferred to a coffee cup calorimeter containing 52.7 g of water (specific heat of 4.184J/g C) initially at 20.63C. if the final temp of the system is 29.59 what was the heat capacity of the calorimeter?

1. A 5.88 kg piece of granite with a specific heat of 0.803 J g-1 °C-1...

1. A 5.88 kg piece of granite with a specific heat of 0.803 J g-1 °C-1 and a temperature of 85.1 °C is placed into 2.00 L of water at 19.0 °C. When the granite and water come to the same temperature, what will the temperature be? 2. The combustion of methane (the chief component of natural gas) follows the equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ∆H° for this reaction is -802.3 kJ. How many grams of methane...

The initial temperature of 140 g of ice is −22°C. The specific heat capacity of ice...

The initial temperature of 140 g of ice is −22°C. The specific heat capacity of ice is 0.5 cal/g·C° and waters is 1 cal/g·C°. The latent heat of fusion of water is 80 cal/g. a. How much heat is required to raise the ice to 0°C? b. How much additional heat is required to completely melt the ice after it has reached 0°C? c. How much additional heat is required to heat the water (obtained by melting the ice) to...

Subjects