### Table 5: Specific Heat of a Metal#### Sample 1**Identity of metal:**- Zinc**[1] Mass of metal (g):**- 20.290 g**[2] Volume of DI water (mL):**- 50.1 mL**Mass of DI water (g):***(Not listed in the table)***[3] Initial temperature of metal (T_initial metal) (°C):**- 96.9 °C**[4] Initial temperature of water (T_initial water) (°C):**- 24.1 °C**[5] Final temperature of the mixture after addition of metal (T_final) (°C):**- 27.1 °C**Specific heat of metal (C_metal) (cal/g·°C):***(Not listed in the table)*This table summarizes the specific heat measurement of zinc. The mass of the zinc sample used was 20.290 grams. The volume of the deionized (DI) water was 50.1 milliliters. The initial temperatures of the metal and the water were 96.9 °C and 24.1 °C, respectively. After mixing, the final temperature of the mixture was 27.1 °C. The specific heat of the metal in cal/g·°C is not provided in the table.

Answered: Image /qna-images/answer/95801cc1-90be-4e9a-a897-2a48d21a8d51.jpg

Table 5. Specific Heat of a Metal Sample 1 Identity of metal Zinc [1] Mass of metal (g) 20.290 [2] Volume of DI water (mL) 50.1 Mass of DI water (g) [3] Tinitial metal (°C) 96.9 [4] Tinitial Water (°C) 24.1 [5] Trinal of mixture after addition of metal (°C) 27.1 Specific heat of metal Cmetal (cal/g-°C)

Table 5. Specific Heat of a Metal Sample 1 Identity of metal Zinc [1] Mass of metal (g) 20.290 [2] Volume of DI water (mL) 50.1 Mass of DI water (g) [3] Tinitial metal (°C) 96.9 [4] Tinitial Water (°C) 24.1 [5] Trinal of mixture after addition of metal (°C) 27.1 Specific heat of metal Cmetal (cal/g-°C)

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...

See similar textbooks

Similar questions

An 8.29 g sample of calcium carbonate [CaCO3(s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. What is the specific heat of calcium carbonate?
2. A solid substance has a mass of 250 grams. It is cooled by 25.00°C and loses 4.937 kJ of heat. What is the specific heat capacity of the substance? 20 3. A 10.0 g sample of pure acetic acid, CH3CO2H, is completely burned. The heat released warms 2.0 L of water from 22.3°C to 39.6°C. I MAR a) Assuming that no heat was lost to the calorimeter, what is the molar enthalpy change of the complete combustion of acetic acid? Express your answer in kJ/mol. b) Will the bonds in the products be longer or shorter than the bonds in the reactants?
A 27.7 g sample of ethylene glycol, car radiator coolant,loses 688 J of heat. What is the initial temperature of the ethylene glycol if the finaltemperature is 32.5 °C (specific heat, c, of ethylene glycol = 2.42 J/g.K?)
A 39.60 g sample of a substance is initially at 23.9 °C. After absorbing 1521 J of heat, the temperature of the substance is 116.6 °C. What is the specific heat (?c) of the substance?
A 35.19 g sample of a substance is initially at 27.1 °C. After absorbing 1533 J of heat, the temperature of the substance is 186.9 °C. What is the specific heat (?) of the substance?
7. An object that has a mass of 75 g is heated from 50°C to 93°C. If it takes 3000 J for the temperature change to occur, then what is the specific heat of the object?