Heat Effects and Calorimetry ### Calorimetry Experiment1. A metal sample weighing 147.90 g and at a temperature of 99.5°C was placed in 49.73 g of water in a calorimeter at 23.0°C. At equilibrium, the temperature of the water and metal was 41.8°C. a. What was Δt for the water? (Δt = t_final - t_initial) **__________ °C** b. What was Δt for the metal? **__________ °C** c. How much heat flowed into the water? (Take the specific heat of the water to be 4.18 J/g°C.) **__________ joules** d. Calculate the specific heat of the metal, using Equation 3. **__________ joules/g°C** e. What is the approximate molar mass of the metal? (Use Eq. 4.) **__________ g/mol**

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1. A metal sample weighing 147.90 g and at a temperature of 99.5°C was placed in 49.73 g of water in a calo- rimeter at 23.0°C. At equilibrium the temperature of the water and metal was 41.8°C. a. What was At for the water? (At = tanal – tinitial) °C b. What was At for the metal? °C с. How much heat flowed into the water? (Take the specific heat of the water to be 4.18 J/g°C.) joules d. Calculate the specific heat of the metal, using Equation 3. joules/g°C e. What is the approximate molar mass of the metal? (Use Eq. 4.) g/mol

1. A metal sample weighing 147.90 g and at a temperature of 99.5°C was placed in 49.73 g of water in a calo- rimeter at 23.0°C. At equilibrium the temperature of the water and metal was 41.8°C. a. What was At for the water? (At = tanal – tinitial) °C b. What was At for the metal? °C с. How much heat flowed into the water? (Take the specific heat of the water to be 4.18 J/g°C.) joules d. Calculate the specific heat of the metal, using Equation 3. joules/g°C e. What is the approximate molar mass of the metal? (Use Eq. 4.) g/mol

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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In a calorimeter, a 75.0 g piece of metal at 98.6 *C is submerged in 100.0 g of water, that is initially at 21.8 *C. When the metal and water reach thermal equilibrium, the temperature is 26.2 *C. What was the heat capacity of the metal (3 sig figs)?
Volume of cool water (mL) Volume of hot water (mL) Initial temperature of cool water (°C) Initial temperature of hot water (°C) Final temperature of water in calorimeter (°C) Temperature change for cool water (°C) Temperature change for calorimeter (°C) Temperature change for hot water (°C) Heat change for cool water (J) Heat change for hot water Heat change for calorimeter (J) Heat capacity of calorimeter (J/°C) Trial 1 50.0 47.5 24.3 38.9 37.0 Trial 2 50.0 46.1 24.9 35.0 33.7 Trial 3 50.0 44.8 23.3 33.8 30.8
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|| Question 15 A calorimeter holds 25 g water at 25.0°C. A sample of hot iron is added to the water, and the final temperature of the water and iron is 30.0°C. What is the change in en- thalpy associated with the change in the water's temperature? Note: The specific heat of water is 4.18 g°c. Use the formula AH = - cm AT %3D Show your work. IUS
I need hand written solution only
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