Suppose 1.16 kg of water at 11.6 ◦C is mixed with 1.7 kg of water at...

Suppose 1.16 kg of water at 11.6 ◦C is mixed with 1.7 kg of water at 81◦C. After equilibrium is reached, the mixture has an uniform temperature of 52.8517◦C. What is the change in entropy of the system? The specific heat of water is 4186 J/kg · K. Answer in units of J/K.

Expert Solution

genius_generous answered 2 years ago

2 kg of iron ingot at 1100oC is mixed with 1 kg of water at -20oC....

2 kg of iron ingot at 1100oC is mixed with 1 kg of water at -20oC. Once the thermal equilibrium is reached, what would be the final state of water? Be as detailed as possible.

4.5kg of water at 25?C is mixed with 4.5kg of water at 58?C in a well-insulated...

4.5kg of water at 25?C is mixed with 4.5kg of water at 58?C in a well-insulated container.Estimate the net change in entropy of the system.

A 50.0-g sample of liquid water at 25.0°C is mixed with 35.0 g of water at...

A 50.0-g sample of liquid water at 25.0°C is mixed with 35.0 g of water at 89.0°C. The final temperature of the water is ________°C.

100 g of ice at -20°C are mixed with 250 g of water at 20°C in...

100 g of ice at -20°C are mixed with 250 g of water at 20°C in an insulated calorimeter. What is the final temperature of the system? How many grams of liquid water and how many grams of ice will you find after the system equilibrates? find T in degrees C; m of solid (in grams); m of liquid (in grams) T=____ ms=____ mliq=____

A cooler contains 1 kg of ice at -5°C. 2 kg of water at 50°C is...

A cooler contains 1 kg of ice at -5°C. 2 kg of water at 50°C is added to the cooler. If the cooler does not exchange any heat with the rest of the world, what is the final temperature of the ice and water?

Steam at 100 °C is bubbled into 2.70 kg of water at 25 °C in a...

Steam at 100 °C is bubbled into 2.70 kg of water at 25 °C in a calorimeter cup. How much steam will have been added when the water in the cup reaches 55 °C? (Ignore the effect of the cup.)

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part...

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part A - Final Temperature What is the final temperature of the system? (If I've set the problem up right, you should be given numbers such that all of the ice has melted.) Tf = ∘C Part B - Entropy of Warming Ice What is the change in entropy of the ice, as it warms up before melting? S = J/K Part C - Entropy...

A: A 2.4 kg pan at 155°C is dumped into 3.5 kg of water at 150...

A: A 2.4 kg pan at 155°C is dumped into 3.5 kg of water at 150 C. What is the change in entropy? B: Q1=50µC, Q2=20µC, Q3=–5µC. What will be the resultant force on Q3? (Q1)-------R1=10cm--------(Q3)-----R2=30cm---------(Q2)

0.7 kg of ice at 0 ◦C and 3 kg of water at Ti are brought...

0.7 kg of ice at 0 ◦C and 3 kg of water at Ti are brought into thermal contact in an iso- lated container. All the ice melts, and the mixture reaches an equilibrium temperature of 10 ◦C. (a) (5 points) Determine the initial temperature Ti of the liquid water. (b) (1 point) Determine the entropy change ∆S_melt associated with this amount of ice melting. (c) (3 points) Determine the entropy change ∆S_coolwater associated with the decreasing temperature of the...

When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C...

When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C water, the final temperature was measured as 40.8 °C. Assume the density for water is 1.000 g/mL regardless of temperature. a. Determine the magnitude of the heat lost by the hot water. b. determine the magnitude of the heat gained by the room temperature water. c. determine the heat gained by the calorimeter d. determine the calorimeter constant.

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