Due: Tomorra All changes saved 2. Why do you cook with metal pots and pans? O Metal has a high heat capacity, which allows it to heat up faster and transfer the heat to the contents of the pot or pan. Metal is a poor conductor of heat. Metals are shiny, and the shininess reflects light, causing it to heat up faster. Metal has a low heat capacity, which allows it to heat up faster and transfer the heat to the contents of the pot or pan. PREVIOUS 2 of 5 NEXTI SAVE & EXIT

Due: Tomorra All changes saved 2. Why do you cook with metal pots and pans? O Metal has a high heat capacity, which allows it to heat up faster and transfer the heat to the contents of the pot or pan. Metal is a poor conductor of heat. Metals are shiny, and the shininess reflects light, causing it to heat up faster. Metal has a low heat capacity, which allows it to heat up faster and transfer the heat to the contents of the pot or pan. PREVIOUS 2 of 5 NEXTI SAVE & EXIT

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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The High Specific Heat Capacity of Water • Water has a high specific heat and is transparent, so it takes more energy to heat up than land does. 20°C 25°C Because water has such a high specific heat capacity, it heats and cools more slowly than land. How does this affect the temperatures on land near bodies of water? O A. It causes land near bodies of water to be much hotter during the day and colder during the night. OB. It helps moderate (not as cold, not as hot) temperatures on land near bodies of water. OC. It causes strong winds to change the amount of rainfall where bodies of water meet the land. OD. It causes the land to give off less heat than the bodies of water they are next to.
A metal X has a a mass of 10.0g and it was heated up to 120.0⁰C, it was then submerged in water that has a mass of 200.0g. The temperature of water increased from 21.0⁰C to 35.0⁰C. Determine the specific heat capacity of metal X. The specific heat capacity of water is 4.18 J/g ⁰C.
An irregular lump of an unknown metal has a measured density of 5.26 g/mL. The metal is heated to a temperature of 183 °C and placed in a graduated cylinder filled with 25.0 mL of water at 25.0 °C. After the system has reached thermal equilibrium, the volume in the cylinder is read at 33.8 mL, and the temperature is recorded as 43.0 °C. What is the specific heat of the unknown metal sample? Assume no heat is lost to the surroundings. C = J g. °C
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)
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Stirring rod A student heats 66.89 grams of platinum to 99.25 °C and then drops it into a cup containing 83.90 grams of water at 22.41 °C. She measures the final temperature to be 24.37.°C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.72 J/°C. Water Assuming that no heat is lost to the surroundings calculate the specific heat of platinum. Metal sample Specific Heat (Pt) =| J/g °C. 02003 Thomeo-BrockaCoe
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
A sample of copper absorbs 44 kJ of heat, resulting in a temperature rise of 65 °C. Determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.
An unknown solid metal at 150 degrees celsius was placed in 1.00 L of water at 25 degrees celsius. The final temperature of the solid metal in the water was 26.3 degrees celsius. In order to find the specific heat of the metal, what additional information is needed?
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?
A 22.0 g piece of metal is heated to 100.0°C and placed in 75.0g of water at 25.0°C. if the final temperature of the metal and water is 27.8°C, what is the specific heat capacity of the metal in J/g°C? The specific heat capacity of water is 4.184 J/g°C. а. 0.038 b. 0.16 c. 0.55 d. 5.0 a
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.
A material has a specific heat of 0.625 J/g°C. A 75.6 g sample of this material is heated and them placed in 35.2 g of water at 21.4 °C. The temperature of the water rises to 32.7 °C. What was the initial temperature of the material?