17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.

17. An ice cube is placed in a sealed insulated container of hot water at 80°C. After five minutes, the ice cube disappears. Ice Cube Heat ener Hot Water 5 min. Water Which best describes the change that took place inside the container? The total heat energy in the container was reduced by the ice cube. The hot water lost the same amount of heat energy as the ice cube gained. in the hot water was reduced by kinetic energy in the ice cube. O Heat energy in the ice cube was dissipated into the hot water.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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18. An unknown volume of water at 18.2°C is added to 24.4 mL of water at 35.0°C. If the final temperature is 23.5°C, what was the unknown volume? (Assume no heat is lost to the surroundings; d of water = 1.00 g/mL)
The table lists the specific heat capacities of select substances. Substance Specific heat capacity (J/g °C) lead 0.128 silver 0.235 0.385 0.449 0.903 4.184 copper iron aluminum water An unknown substance has a mass of 18.9 g. The temperature of the substance increases by 16.5 °C when 73.3 J of heat is added to the substance. What is the most likely identity of the substance? water Olead O copper iron. silver aluminum
Calculate the amount of heat (in kJ) required to raise the temperature of a 0.169 kg sample of ethanol from 298.0 K to 367.4 K. The specific heat capacity of ethanol is 2.42 J/g°C. a. 73.6 kJ b. 12.9 kJ c. 57.0 kJ d. 16.6 kJ e. 28.4 kJ
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4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)
8. Heat is applied to 50g of water (specific heat of 4.18J/°C) at 25°C. The temperature of the water increases to 98°C. What was the total amount of heat energy that was applied?
A hot 122.8 g lump of an unknown substance initially at 154.8 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is allowed to reach thermal equilibrium. The final temperature of the system is 56.9 °C. Using this information and the specific heat values for several metals in the table, identify the unknown substance. Assume no heat is lost to the surroundings. graphite zinc aluminum titanium tungsten rhodium Substance Specific heat (J/(g-°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 0.132 0.388 4.184 tungsten zinc water
4. The heat capacity of copper is 0.382 J/g°.C. A 22.6 g sample of copper at 93° C is placed in 50 g of water at 23.9° C. What is the final temperature of the system?
A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of copper will heat the water to the lowest final temperature? The specific heat of copper is 0.385 J-g-1.°C-1. The specific heat of water is 4.184 J·g-1.°C-1. A. 5.0 g Cu B. 2.0 g Cu C. 0.5 g Cu D. 1.0 g Cu
An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water at 21.0°C The contents of the calorimeter come to a temperature of 25.7°C. The heat capacity of water is 4.18 J/(g* °C) a. Is this process exothermic or endothermic? b. Calculate the amount of heat released by the metal (q metal) in Joules. Show your work.
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.