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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When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure calorimeter. The initial temperature of both solutions is the same at 17.35°C, and the final temperature of the mixed solution is 19.02°C. What is the heat capacity of the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.
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
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
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 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.
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
A 47.70 mL volume of 1.00 M HCl was mixed with 47.30 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.0 J/°C) at 21.71 °C. The final temperature of the aqueous solution after the reaction was 29.73 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) in kJ/mol HCl
Consider the change in the internal energy of a system. what is the change in the internal energy, in joules, of a system that does 4.75 x 10^5 J of work, while 3.05 x 10^6J of heat is transferred into the system and 8.25 x 10^6J of heat is transferred from the system to the environment?