Use the table of specific heat capacities below to answer this question.A 10 g sample of each substance is placed in a -20°C freezer for 10 minutes. Whichsample undergoes the smallest change in temperature?Specific Heat(J/g°C)SubstanceWood1.76Aluminum 0.902Concrete0.88Iron0.451Copper0.385Lead0.129

Given, equal mass(10 g) of each substances are placed in the freezer for the same amount of time at…

Answered: A 10 g sample of each substance is…

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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A 52.0 g sample of polystyrene is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The polystyrene sample starts off at 86.4 °C and the temperature of the water starts off at 21.0 °C. When the temperature of the water stops changing it's 26.0 °C. The pressure remains constant at 1 atm. Calculate the specific heat capacity of polystyrene according to this experiment. Be sure your answer is rounded to 2 significant digits. đặc J g. °C 0 x10 X thermometer insulated. container water sample a calorimeter
A piece of metal with a mass of 59.047 g was heated to 98.0°C and then put into 100.0g of water initially at 23.7°C. The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heat (J/g•°C) of the metal.
Which statement best defines specific heat? The amount of heat required to increase the temperature of 1 mol of a substance by 1 °C. The amount of heat required to increase the temperature of a specific object, such as a calorimeter, by 1 °C. The amount of heat required to increase the temperature of 1 g of a substance by 1 °C. The amount of heat required to increase the temperature of 1 L of a substance by 1 °C.
A candy bar has a total mass of 75.0 grams. In a calorimetry experiment, a 1.25-g sample of this candy bar was burned in a calorimeter surrounded by 1000 g of water. The temperature of the water in contact with the burning candy bar was measured and found to increase from an initial temperature of 21.2°C to a final temperature of 24.3°C. a. Calculate the amount of heat in calories released when the 1.25-g sample burned. (show the work you did)
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
You have a sample of water with an unknown amount of mass. You add 348J of heat to the sample and measure the change in temperature to be increasing by 5.2 degrees celsius. What is the mass of the sample of water? The specific heat of water is 4.18 J/(g x degrees Celsius).
Which substance will have the largest temperature change if the same amount of heat is added to each of them?Gold, Au(s): specific heat = 0.0308 calories per gram degree Celsius.Water, H2O(l): specific heat = 1.00 calorie per gram degree Celsius.Copper, Cu(s): specific heat = 0.0920 calorie per gram degree Celsius.Ethanol, C2H5OH(l): specific heat = 0.588 calorie per gram degree Celsius
How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.
If the specific heat of methanol is 2.51 j/k-g, how many joules are required to raise the temperature of 50 g of methanol from 20oc to 70oc?
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 silver cube with an edge length of 2.36 cm and a gold cube with an edge length of 2.75 cm are both heated to 87.5 ∘C and placed in 105.0 mL of water at 20.2 ∘C . What is the final temperature of the water when thermal equilibrium is reached? Substance Specific heat (J/g·°C) Density (g/cm3) gold 0.1256 19.3 silver 0.2386 10.5 water 4.184 1.00 A silver cube with an edge length of 2.36 cm and a gold cube with an edge length of 2.75 cm are both heated to 87.5 ∘C and placed in 105.0 mL of water at 20.2 ∘C . What is the final temperature of the water when thermal equilibrium is reached? ?final=
A hot 101.7101.7 g lump of an unknown substance initially at 184.9184.9 °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 86.486.4 °C. 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 4.184 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. a) zinc b) graphite c) titanium d) tungsten e) rhodium f) aluminum

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A 10 g sample of each substance is placed in a -20°C freezer for 10 minutes. Which sample undergoes the smallest change in temperature? Substance Specific Heat