A chemist heats the block of silver as shown in the interactive, then places the metal sample in a cup of oil at 25.00 °C insteadof a cup of water. The temperature of the oil increases to 27.05 °C. Calculate the mass of oil in the cup. The specific heat ofsilver is 0.234 J/g °C and the specific heat of oil is 1.74 J/g - °C..moil =go

Since, the mass and temperature of silver after being heated is not given. We can assume a…

Answered: A chemist heats the block of silver as…

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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A piece of metal weighing 100 g was heated to 43.85 °C. (Initial temperature of metal was 23 ° C). The metal was placed in 50g of water and the temperature of the water changed from 18 ° C to 23 ° C. Find the specific heat for this metal. (Specific Heat of Water (C) = 4.184 J/g° C) %3D
A 90.0 g piece of metal, initially at 98.6°C, is placed into 120.0 g of water initially at 24.3°C. If the final temperature of the water is 34.0°C, what is the specific heat of the metal? (The specific heat of water is 4.18 J/g･°C).
A 55.0 g sample of nickel (specific heat = 0.433 J/g°C) at 100.0°C is added to 65.0 g of water at 25.0°C. What is the final temperature of the water and the metal?
A piece of plastic at 161 degree C was put in a beaker with 105.9 g ethanol at 20.5 degree C . The temperature of the water rose to 39 degree C. Given that the specific heat of ethanol is 2.46 J/g degree C, what is the heat capacity of the piece of plastic in J/degree C? Use proper sig figs. Gracias!
A student heated a 56.0000 g metal object to 97.3 °C and transferred it to a calorimeter containing 100.4300 g of water at 25.2 °C. The water and metal reach a final temperature of 26.5 °C. How much heat did the metal release? (specific heat of water: 4.186 J/g°c) Select one: 0.30 kJ 17 kJ 30 kJ 0.55 kJ
The freezing point of mercury is -38.8 degrees Celsius. What Energy is released to the surroundings if 1 ml of mercury is cooled from 23 to 38 degrees Celsius and then frozen to solid? Density of Mercury is 13.6 g/ml, specific heat capacity is 0.140 j/gK and its heat of fusion is 11.4½.
A piece of metal weighing 146.7 g was heated from 32.0 °C to 56.2 °C. If the amount of heat needed was 1363.3 J, calculate the specific heat of the metal. What is the identity of the metal? 20 Specific Heats of Selected Metals Smetal, J/g-°C Metal 0.901 Smetal, J/g-°C 0.449 Metal Al Fe Cu 0.384 Ni 0.444 Si 0.711 Sn 0.226 Zn 0.389 Mn 1.02
Aluminum and iron samples, each weighing 2 kg, absorb 11.5 kJ of heat. Which material would have the greatest change in temperature? Considering that aluminum has a specific heat capacity of 0.89 J/g K) and iron has 0.45 J/g K.
A 147.1 g piece of copper (specific heat 0.380 J/g･ °C) is heated and then placed into 400.0 g of water initially at 20.7 °C. The water increases in temperature to a final temperature of 22.2 °C. What is the initial temperature (in °C) of the copper? (The specific heat of water is 4.184 J/g･ °C).
A 5.0 g sample of water starting at 59.4°C loses 439 J of energy in the form of heat. What is the final temperature of the water after this heat loss? The specific heat for water is 4.18 J/(g.°C). Temperature = °C
3. We all know that the hood of a car gets extremely hot in the summertime when a bright sun is shining on it. Suppose that a certain hood weighs 22.8 pounds and is composed of pure iron. If the specific heat of the iron is 0.450 J/g °C, what is the final temperature of the hood if it is heated from 20.0 °C by the addition of 4.0 x 102 kJ of sunlight? (Recall that 1 pound = 0.4536 kg)
A 2.50 g sample of zinc is heated, then placed in a calorimeter containing 65.0 g of water. Temperature of water increases from 20.00 °C to 22.50 °C. The specific heat of zinc is 0.390 J/g°C. What was the initial temperature of the zinc metal sample? (final temperatures of zinc and water are the same)

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