The specific heat capacity of a pure substance can be found by dividing the heat needed to change the temperature of a sample of the substance by the mass of J g.°C the sample and by the change in temperature. The heat capacity of a certain substance has been measured to be 4.78 are heated until the temperature of the sample has changed by 6.42 °C. Suppose 189. g of the substance Write an equation that will let you calculate the heat Q that was needed for this temperature change. Your equation should contain only symbols. Be sure you define each symbol. Your equation: Definitions of your symbols: J g. °C 0 = 4.78 = 189. g = 6.42 °C olo 0 X E A S

The specific heat capacity of a pure substance can be found by dividing the heat needed to change the temperature of a sample of the substance by the mass of J g.°C the sample and by the change in temperature. The heat capacity of a certain substance has been measured to be 4.78 are heated until the temperature of the sample has changed by 6.42 °C. Suppose 189. g of the substance Write an equation that will let you calculate the heat Q that was needed for this temperature change. Your equation should contain only symbols. Be sure you define each symbol. Your equation: Definitions of your symbols: J g. °C 0 = 4.78 = 189. g = 6.42 °C olo 0 X E A S

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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2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
2. A sample of nickel is heated to 99.8°C and placed in a coffee cup calorimeter containing 150.0 g water at 23.5°C. After the metal cools, the final temperature of metal and water mixture is 25.0°C. If the specific heat capacity of nickel is 0.444 J/°C a. what mass of nickel was originally heated? Assume no heat loss to the surroundings.
A 29.00 g sample of metal alloy is heated to 92.6 °C; then placed in 55.23 g of water in an insulated calorimeter at 21.3 °C. If the final temperature of the system is 43.9 °C, what is the specific heat of the metal alloy? Assume that the calorimeter absorbs a negligible amount of heat.
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A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś
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