stry-S2 - MI / Thermochemistry/Lesson 159 20. Specific heat is defined as O the amount of energy needed to raise the temperature of a substance by 1° C the amount of energy needed to raise the temperature of 1 gram of a substance by 1° C the amount of energy needed to raise the temperature of water by 1° C the amoint of energy needed to raise the temperature of 1 gram of a substance by 1° K

stry-S2 - MI / Thermochemistry/Lesson 159 20. Specific heat is defined as O the amount of energy needed to raise the temperature of a substance by 1° C the amount of energy needed to raise the temperature of 1 gram of a substance by 1° C the amount of energy needed to raise the temperature of water by 1° C the amoint of energy needed to raise the temperature of 1 gram of a substance by 1° K

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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An experiment was conducted to determine the specific heat of platinum. It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC. Based on these experimental results calculate the specific heat (J/goC) of platinum. Do not type units into your answer.
How many joules of energy are needed to raise the temperature of an item 55 degrees if the heat capacity of the item is 259 J/"C? O 20400J O 314J O 14245 J O 4.7J Question 4 What temperature change would you expect if you have an object that has a specific heat capacity of 982 J/g.°C, a mass of 75.2 grams, and it released 3476.2 joules of heat. O 47.1 K O 47.1 K O -45 K O 45 K Question 9 For the same substance, the enthalpy of fusion is much lower than the enthalpy of vaporization (fusion= 6.02 kJ/mol and vaporization= 40.65 kJ/mol). What would be the correct full explanation for why this occurs? O When you melt a solid into a liquid, you need to completely overcome the intermolecular forces holding the molecules together O When you vaporize a liquid, you have to break bonds O When you turm a liquid into a gas, you need to completely overcome the intermolecular forces holding the molecules together O When you melt a solid into a liquid, you need to break the bonds
If a 50.0 g piece of brass rod at 98.0°C is placed in 150.0 g of water at 25.0°C, what is the final temperature? Assume that no heat is transferred to the surroundings. The specific heat capacity of water is 4.18 J/g °C. The specific heat capacity of brass is 0.38 J/g °C. 35 79 42 27
If 1495 J of heat is needed to raise the temperature of a 357 g sample of a metal from 55.0°C to 66.0°C, what is the specific heat capacity of the metal?______ J/g•°C
In the laboratory a student determines the specific heat of a metal.He heats 18.4 grams of platinum to 99.28 °C and then drops it into an insulated cup containing 85.3 grams of water at 23.56 °C. When thermal equilibrium is reached, he measures the final temperature to be 24.10 °C.Assuming that all of the heat is transferred to the water, he calculates the specific heat of platinum to be J/g°C.
You heat 26.1 g of a solid in a test tube to 100.00°C and add it to 50.00 g of water in a coffee-cup calorimeter. The water temperature changes from 20.2°C to 28.49°C. Find the specific heat capacity of the solid. c of water = 4.184 J/gK Enter to 3 decimal places.
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.61 kg sample of a pure substance from 3.0 °C to 24.2 °C. The experiment shows that 32. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. 1 - 1 ·K x10
A Chemistry 1A student drops 105.0 grams of copper with an initial temperature of 95.4 °C into a coffee cup calorimeter containing 100.0 grams of water. The water in the calorimeter was initially at 23.5 °C before the copper was added. Assuming no heat is lost to the environment, what will be the final temperature (°C) of the water?
A 88.8 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 24.8°C. Ignoring significant figures, calculate the mass of water in the calorimeter.
a 90.00g piece of metal is placed in water and the water gains 1230 J of heat as the temperature of the metal changes by 59.0 C. calculate the specific heat capacity of the metal
If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?
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