A 237-g piece of iron, initially at 100.0 °C, is dropped into 244 g of water at 10.0 °C. When the system comes to thermal equilibrium, the temperature is 18.5 °C. What is the specific heat capacity of iron? The specific heat capacity of water is 4.184 J/g K. Specific heat capacity: Submit Answer 9 more group attempts remaining Retry Entire Group J/g. K

A 237-g piece of iron, initially at 100.0 °C, is dropped into 244 g of water at 10.0 °C. When the system comes to thermal equilibrium, the temperature is 18.5 °C. What is the specific heat capacity of iron? The specific heat capacity of water is 4.184 J/g K. Specific heat capacity: Submit Answer 9 more group attempts remaining Retry Entire Group J/g. K

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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6. Determine the mass of a sample of water in a coffee cup calorimeter if the final temperature is 65.7 °C, the initial temperature is 22.3 °C, and 27.6 kJ of heat is added to the water (specific heat of water is 4.184 J/g•K).
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 30.00 g sample of a solid was heated in a test tube to 100.00o C in boiling water and carefully added to a coffee cup calorimeter containing 40.00g of water. The water temperature increased from 25.00o C to 29.50o C. What is the specific heat capacity of the solid? (Assume all the heat is gained by the water) The heat capacity of water is 4.18 J/(go C)
Iron has a specific heat capacity of 0.444J/g-C. 50.0 g of iron at 35C is added to 50.0 g of water with a specific heat capacity of 4.184 J/g-C. When the temperature of the resulting mixture stops changing, the temperature is closer to that of the original water than to the iron. True or false?
A 19.3 g sample of beryllium at 96.7°C is placed into 46.2 mL of water at 20.2°C in an insulated container. The temperature of the water at thermal equilibrium is 32.0°C. What is the specific heat of beryllium? Assume a density of 1.00 g/mL for water. (See this table.) J/(g·°C)
The temperature of an object increases by 43.5 °C when it absorbs 3829 J of heat. Calculate the heat capacity of the object. C = The mass of the object is 367 g. Use the table of specific heat values to identify the composition of the object. Substance Specific heat (J/(g. °C)) gold 0.129. silver 0.240 iron 0.444 aluminum 0.900 The object is composed of O aluminum. silver. gold. iron. J/°C
A glass contains 250.0 g of warm water at 78.0°C. A 50.0 g piece of gold at 2.30°C is placed in the water. What is the final temperature reached by this system? The specific heat of water is 4.184) g1 °C1, and that of gold is 0.129J g1 °C1. A 78.45°C B 76.36°C c) 79.63°C D 77.54°C
A 46-g sample of liquid water at 25.0 C is mixed with 22 g of water at 45.0°C. The final temperature of the water is ________°C. The specific heat capacity of liquid water is 4.18 J/g-K.
H8. A student combined 107.5 mL of 0.2400 M HCl and 127.9 mL of 0.3650 M NaOH in a calorimeter of negligible heat capacity . The reactants were initially at 27.1 degrees Celsius. Determine the final temperature this mixture should reach in degrees Celsius (oC), given that the heat of neutralization of this reaction is -56.2 kJ/1 mol water, the specific heat capacity of water is 4.184 J/(g.oC) and assuming that the density of all the solutions is 1.00 g/mL (Hint: The reaction between an acid and a base produces a salt and water)
A silver block, initially at 51.0 °C, is submerged into 100.0 grams of water at 25.3 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 28.0°C. What is the mass of the silver block? The specific heat capacity of silver is 0.235 J/g°C The specific heat capacity of water is 4.184 J/g°C Do not type units with your answer. Type your answer to four significant figures. If this question is on an exam on your scrap paper report your answer to the proper number of significant figures but still type four significant figures online.
1. ethylene glycol 2. Substance 3. brass glass 4. vegetable oil Specific Heat Capacity (J/g °C) 2.47 I 0.377 0.837 1.97 A 50 g sample of each of the above materials, each with an initial temperature of 21.0°C, had the same quantity of thermal energy added to them. If they were listed from the highest final temperature reached to the lowest final temperature reached, the order would be ◆ and ◆ I 660 kJ of thermal energy are added to 2000 g of vegetable oil in a fondue pot. The vegetable oil had an initial temperature of 21.3 °C. Assume that the thermal energy absorbed by the fondue pot is negligible. The final temperature of the vegetable oil would be °C. Record your 3-digit answer; do not include units.
A 39.7 g block of an unknown metal at 97.2°C is placed into 500.0 g of water initially at 17.0°C and has a final temperature of the water and the metal of 24.2°C. What is the specific heat capacity of the unknown metal in J/g･°C? The specific heat capacity of water is 4.184 J/g･°C.