Question

Hot water added to cold water spontaneously mixes so that all of the water has the...

Hot water added to cold water spontaneously mixes so that all of the water has the same average temperature. State and apply the laws of thermodynamics to explain this process.

Homework Answers

Answer #1

LAW OF CONSERVATION OF ENERGY

Adding equal amounts of hot water and cool water produces a final temperature halfway between the initial temperatures of both. When the proportions of the hot and cold water were varied, the temperature changed. The final temperature was somewhere between the two initial temperatures, and nearer to the temperature of the water with the larger mass. The law of conservation of energy informs us that if the cold water gained thermal energy through the transfer of heat, then the hot water must have lost an equal amount of thermal energy. The total energy change must be zero. An equation to express this might look as follows:

Δ Qh + ΔQc =0

mh (Tf -Th) + mc (Tf -Tc) =0

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A student mixes 100ml of hot water (90degrees) with 50ml of cold water (15 C) what...
A student mixes 100ml of hot water (90degrees) with 50ml of cold water (15 C) what is the final temperature of the mixture?
a. An ice cold piece of aluminum metal is added to 50.0 g of hot water....
a. An ice cold piece of aluminum metal is added to 50.0 g of hot water. Given the average initial temperature (76 C) calculated above for the hot water, calculate the heat, q, in joules of the piece of aluminum metal if the final temperature of the water is 40.0 °C. The specific heat of water is 4.184 J/g-°C. (0.50) b. Calculate the grams of aluminum metal used if the specific heat of aluminum is 0.895 J/g-°C. (0.50)
Hard/ Soft water: Why is CaCO3 present in hot water, but not in cold? My prfoessor...
Hard/ Soft water: Why is CaCO3 present in hot water, but not in cold? My prfoessor talked about he has his water softerner only for hot water, but the cold water is not passed through a water softner. Can you please explain showing step by step equilibrium reactions and where the equilibrium is favored. Here are a few equations that might help your thought process. I guess I would just like an explaination as to why hot vs cold and...
Exactly 17.7 mL of water at 35.0 °C are added to a hot iron skillet. All...
Exactly 17.7 mL of water at 35.0 °C are added to a hot iron skillet. All of the water is converted into steam at 100.0°C. The mass of the pan is 1.20 kg and the molar heat capacity of iron is 25.19 J/(mol·°C). What is the temperature change of the skillet?
For any system that may undergo any process, we expect the process to occur spontaneously only...
For any system that may undergo any process, we expect the process to occur spontaneously only if ∆Guniverse<0. For a chemical system that may react,∆G sys=RTln(Q/K), so under standard state conditions (where [X]º=1 M and Px=1 atm) ∆Gsys=∆G°= RTln(1/K)= –RTlnK. Thus, at equilibrium (whereQ=K), ∆G= RTln(1) = 0. Use these ideas to explain why the laws of thermodynamics predict that no chemical reaction in a closed system should ever go to 100% completion.
Select each of the 0th, 1st, and 2nd laws of thermodynamics. Don't pick the false statements....
Select each of the 0th, 1st, and 2nd laws of thermodynamics. Don't pick the false statements. Group of answer choices an expanding gas will always increase in temperature If system A is in thermal equilibrium with system B, and system B is in thermal equilibrium with system C, systems A and C are also in thermal equilibrium. Work can never be done when heat is transferred from a hot to a cold reservoir. The work created by a heat engine...
For any system that may undergo any process, we expect the process to occur spontaneously only...
For any system that may undergo any process, we expect the process to occur spontaneously only if ∆Guniverse <0. For a chemical system that may react, ∆Gsys = RT ln(Q/K), so under standard state conditions (where [X] º 1 M and PX º 1 atm) ∆Gsys = ∆G° = RT ln(1/K) = –RT lnK. Thus, at equilibrium (where Q = K), ∆G = RT ln(1) = 0. Use these ideas to explain why the laws of thermodynamics predict that no...
Using terminology from Chapter 10, explain how a cold water bath could feel warm. Terms from...
Using terminology from Chapter 10, explain how a cold water bath could feel warm. Terms from Chapter 10: Temperature Thermal Equilibrium Zeroth law of thermodynamics absolute zero absolute temperature specific heat capacity change of phase latent heat first law of thermodynamics internal energy conduction thermal conductivity convection radiation * Not all terms have to be used*
Exactly 10.8 mL of water at 30.0 degrees C are added to a hot iron skillet....
Exactly 10.8 mL of water at 30.0 degrees C are added to a hot iron skillet. All of the water is converted into steam at 100 degrees C. The mass of the pan is 1.20 kg and the molar heat capacity of iron is 25.19 J/(mol*degrees C). What is the temperature change of the skillet?
Exactly 14.1 mL of water at 31.0 degrees C are added to a hot iron skillet....
Exactly 14.1 mL of water at 31.0 degrees C are added to a hot iron skillet. All of the water is converted into steam at 100 degrees C. The mass of the pan is 1.45 kg and the molar heat capacity of iron os 25.19 J/(mol degrees C). What is the temperature change of the skillet?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT