An experiment was performed to determine the heat capacity of a coffee cup calorimeter. The calorimeter contained 90.0 g of water at a temperature of 21.3°C. 105.0 g of water at a temperature of 50.2 °C were poured into the calorimeter and the contents of the calorimeter were stirred The final temperature of the water and the calorirmeter was 35.6 °C. The specific heat capacity of water is 4.184 J/g.°C. What is the heat capacity of the

An experiment was performed to determine the heat capacity of a coffee cup calorimeter. The calorimeter contained 90.0 g of water at a temperature of 21.3°C. 105.0 g of water at a temperature of 50.2 °C were poured into the calorimeter and the contents of the calorimeter were stirred The final temperature of the water and the calorirmeter was 35.6 °C. The specific heat capacity of water is 4.184 J/g.°C. What is the heat capacity of the

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 reaction of zinc with hydrochloric acid is represented by the reactionZn(s) + 2 HCl(aq) ↔ ZnCl 2(aq) + H 2(g) -- ΔH = -152.5 kJ How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0Â°C to 35.85 Â°C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
When pure sulfuric acid is dissolved in water, heat is evolved. 10.65 g of pure sulfuric acid at 20.00 °C was added to a calorimeter containing 300 g of water at 20.00 °C. The temperature of the solution increased to 26.35 °C. If the specific heat of the mixture is 4.184 Jg1°C1, the density of water is 1 g/mL, and the heat capacity of the calorimeter is ignored, what is the heat evolved per mole of sulfuric acid? a. -83.2 kJ O b. -73.6 kJ O C. -76.0 kJ d. -80.8 kJ e. -78.4 kJ
calculate the heat (in J) of the reaction if 50.0 mL of HCl is added to 50.0 mL of NaOH in a coffee-cup calorimeter. The initial temperature for both solutions is 23.2oC. At the end of the reaction after the data is graphed, the final temperature is determined to be 38.5oC.
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
A 2.74 g sample of methanol, CH3OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 10.1°C. If the heat capacity of the bomb is 727.1 J/°C and it contains 1200 kg of water, what is the heat evolved in kJ/mol of methanol combusted? The specific heat capacity of water is 4.184 J/g°C and the molar mass of methanol is 32.04 g/mol. Show your answer in TWO (2) decimal places.
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a chemist wastes a delicious brownie by burning it in a bomb calorimeter. before burning, the brownie weighed 16.13 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.40 degrees celsius. The known heat capacity of the calorimeter that was used was 26.53 kJ/Celsius. What is the energy content, in kJ/g, of this brownie?
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An 8.0 g sample margarine was placed in a bomb calorimeter. It was then completely combusted leading to a temperature change of 36.18 °C. The heat capacity of the calorimeter was previously determined to be 7.25 kJ/kg°C. What was the quantity of heat released to the environment by the sample of margarine?
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol
A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C