Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- When immersed in water, the temperature of a 102.1 gram sample of metal changes from 150.2 0C to 45.2 0C. During this temperature change, the heat of the metal was -10,161 joules. Calculate the specific heat capacity of the metal.arrow_forwardThe specific heat of a substance is the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius. The relationship between the amount of heat gained or released by a substance and the change in temperature of the substance is given by the equation ?=??Δ?q=msΔT where ?q is the heat gained or released, ?m is the mass of the substance, ?s is the specific heat of the substance, and Δ?ΔT is the change in temperature. 1. Rearrange the equation to solve for ?. 2. When a substance with a specific heat of 0.635 J/g⋅∘C0.635 J/g⋅∘C is heated from 25.2 ∘C25.2 ∘C to 71.4 ∘C,71.4 ∘C, it absorbs 422 J422 J of heat. Calculate the mass of the substance.arrow_forwardA 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is reached. The sample is quickly transferred to 55.604 g of water at 22.6°C contained in a calorimeter. When thermal equilibrium is reached the temperature of the water is measured to be 27.3°C. What is the specific heat of the metal? Specific heat of water is 4.184 J/ grams•°C In part A, (metal-water ) how was the initial temperature of WATER determined? In part A, (metal-water ) how was the initial temperature of METAL determined?arrow_forward
- 4. A 505 gram piece of copper tubing is heated to 99.0 °C and placed in an insulated vessel containing 59.8 grams of water at 24.8 °C. Assume that the water and the vessel are at the same temperature and that all of the heat released from the copper is absorbed by the water and the vessel. If the vessel has a heat capacity of 10.0 J/K, what is the final temperature of the system when it reaches physical equilibrium?arrow_forwardA sample of copper was heated to 120o C and then plunged into an insulated vessel containing 200.g of water at 25.00o C. The final temperature of the mixture was 26.50o C. Assuming no heat was lost to the surroundings, calculate the mass of the copper sample. The specific heat of copper is 0.385 J/go C and the specific heat of water is 4.184 J/go C.arrow_forwardA 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J respectively. g• °C 0.387 g• °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine th heat capacity of the calorimeter. Heat capacity of calorimeter =arrow_forward
- A sample of copper with a specific heat of 0.385 J goC is heated from 45.6 oC to 80.7 oC. What is the mass of the copper sample if this process required 816.24 J of energy?arrow_forwardA hot 105.9 g lump of an unknown substance initially at 154.0 °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 36.2 °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. rhodium ○ graphite titanium zinc tungsten aluminum Substance Specific heat (J/(g∙°C)) aluminum 0.897 graphite 0.709 rhodium 0.243 titanium 0.523 tungsten 0.132 zinc 0.388 water 4.184arrow_forwardA particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.arrow_forward
- In an experiment, 26.5 g of metal was heated to 98.0°C and then quickly transferred to 150.0 g of water in a calorimeter. The initial temperature of the water was 22.5°C, and the final temperature after the addition of the metal was 32.5°C. Assume the calorimeter behaves ideally and does not absorb or release heat.arrow_forwardCalculate the heat of reaction (in J)arrow_forward152 A 352.44 Your Answer: 155 T 362.31 Answer 153 units Gö G D 355.67 156 X 154 365.88 359.12 157 You time travel 100 years into the future and learn that several new elements have been discovered, as pictured. These elements are frequently found as oxides, and need to be separated in order to extract the pure element. Before going through this effort, it is useful to know what amount of the element can be extracted. How many moles of element A can be extracted from 175 grams of A5012? N 369.52arrow_forward
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