Part A Substances A and B, initially at different temperatures, come in contact with each other and reach thermal equilibrium. The mass of substance A is twice the mass of substance B. The specific heat capacity of substance A is twice the specific heat capacity of substance B. Which statement is true about the final temperature of the two substances once thermal equilibrium is reached? O The final temperature will be exactly midway between the initial temperatures of substances A and B. O The final temperature will be closer to the initial temperature of substance A than substance B. O The final temperature will be closer to the initial temperature of substance B than substance A

Part A Substances A and B, initially at different temperatures, come in contact with each other and reach thermal equilibrium. The mass of substance A is twice the mass of substance B. The specific heat capacity of substance A is twice the specific heat capacity of substance B. Which statement is true about the final temperature of the two substances once thermal equilibrium is reached? O The final temperature will be exactly midway between the initial temperatures of substances A and B. O The final temperature will be closer to the initial temperature of substance A than substance B. O The final temperature will be closer to the initial temperature of substance B than substance A

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...

See similar textbooks

Similar questions

If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the largest temperature change? Metal Specific Heat Capacity (J/g-K) A 0.753 B 0.129 C 0.385 D 0.449 E 0.897
1.Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g of water at 10.0 °C. Object A increases the water temperature by 3.50 °C; B increases the water temperature by 2.60 °C. a. Which object has the larger heat capacity? b. What can you say about the specific heats of A and B?
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
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.
Material A and material B was exposed to the same change in temperature- but the heat involved with A is 3 times greater than B. If mass of A is 1 kg and mass of B is 10 kg. how do you describe their specific heat ? * O Specific heat of A is 10 times lesser compared to B O Specific heat of A is 10 times greater compared to B O Specific heat of A is 20 times greater compared to B Specific heat of A is 30 times greater compared to B
A 25.09 g sample of a substance is initially at 24.0 °C. After absorbing 2121 J of heat, the temperature of the substance is 124.5 °C. What is the specific heat (?) of the substance?
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
A sheet of metal weighing 275-g is heated to 100.0 °C and placed flat in 100.00 g bucket of water at 22.0 °C. What is the final temperature of the combined substances? Assume that no heat is lost to the surroundings. The specific heat capacity of the metal is 0.444 J/g.°C . The specific heat of water is 4.184 J/g.°C. Select one: O a. 61.0 °C Оъ. 82.4 °С O c. 79.2 °C d. 40.8 °C × О е. 39.6 °C
Two portions of 50.0 g of water, at 13.0 and 55.0 °C, respectively, were mixed inside a cup calorimeter. If the temperature of water after mixing became 31.0 °C, Calculate the heat capacity of the calorimeter. Given that specific heat of water is 4.184 J/ *C.g. a. 34.9 J/°C b. 69.7 J/°C c. 58.1 J/°C d. 23.2 J/°C e 46.5 J/C
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