A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)

A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)

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

Related questions

Q: A 20.0 g block of iron (molar heat capacity 25.1 J/mol °C) at 83.4 °C is placed into 200.0 g of…

A: Answer:This question is based on law of conservation of energy where energy lost by hotter object…

Q: Calculate the amount of heat (in kJ) required to raise the temperature of 1.65 lb of water from 294K…

A: Given : Initial temperature = 294K Final temperature = 303K Mass of water = 1.65lb

Q: A 110.0-g sample of a gray-colored, unknown, pure metal was heated to 92.0 oC and put into a…

A: Assuming specific heat of metal is C. Since all the heat released by metal in reaching the final…

Q: How much heat is required to raise the temperature of a 1.15 kg piece of copper metal from 25.0 °C…

A: Given :- Mass of Copper metal = m = 1.15 kg = 1150 g Initial temperature of Copper metal = Ti =…

Q: A 28.3-g piece of iron initially at 84.4 °C is submerged into 107.2 g of water at 12.2 °C. What is…

Q: A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if…

A: Q. Given Gold (Au ) sample m = 28.5 g (given mass of gold ) Qr = - 0.157 kJ = -157 J (Heat released…

Q: A 4.22 kg piece of copper metal is heated from 20.5°C to 224.5°C. Calculate the heat absorbed (in…

A: The mass of 1.0 kg in g is 1000 g. The mass of the 6.22 kg copper in g is 6220 g. 1000 g=1.0 kg 4.22…

Q: The specific heat capacities of copper, gold, and cobalt are given. Based on this information, which…

A: Specific heat capacity means the amount of heat required to raise the temperature of 1 gram of a…

Q: When 110. g of water at a temperature of 22.3 °C is mixed with 65.9 g of water at an unknown…

A: The final temperature is achieved at equilibrium. According to law of conservation of energy, the…

Q: Aluminium is a silvery-white light-weight metal that is soft and malleable. A 215.0 g piece of…

Q: A 149.5-g sample of a metal at 75.5°C is added to 149.5 g H₂O at 15.6°C. The temperature of the…

A: Mass of Water, m = 149.5 gspecific heat of water, s = 4.184 J/goCinitial temperature, T1 = 15.6…

Q: A 13.8 g piece of nickel was heated to 97.5 °C in boiling water and then dropped into a beaker…

Q: A 50.0-g block of an unknown substance initially at 177.39 °C was submerged in 40.0 mL of water…

Q: A 148.8-g sample of a metal at 74.0°C is added to 148.8 g H2O at 15.5°C. The temperature of the…

A: Specific heat- It is the amount of heat required to raise the temperature of 1g of substance by 10…

Q: An experiment was conducted to determine the specific heat of platinum. It was determined that…

A: Heat required to raise the temperature = 158.8 Joules. Mass of a sample = 50.0 g Initial…

Q: A 148.9-g sample of a metal at 74.0°C is added to 148.9 g H20 at 14.4°C. The temperature of the…

Q: You add 100.0 g of water at 58.3 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools…

Q: A 151.8-g sample of a metal at 74.0°C is added to 151.8 g at 15.8°C. The temperature of the water…

A: Given : Mass of water = 151.8 g Mass of metal = 151.8 g Initial temperature of water = 15.8 oC Final…

Q: 58.2 g sample of Sn metal at 91.1°C was dropped into 70.4 g of H2O at 20.7°C, and after the…

A: We will use calorimetry principle

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g °C) at 34.0 °C is placed into 500.0 g of…

A: We have to calculate the change in temperature for metal block.

Q: A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of…

A: Given,Mass of iron (m1) = 25 gInitial temperature of iron (Ti) = 398 KSpecific heat capacity of iron…

Q: A 25.0 g block of copper (specific heat capacity 0.380 J/g °C) at 99.4 °C is placed into 500.0 g of…

A: Q = m . s . ΔT Where, Q = heat absorbed or evolved; m = mass of substance; s = specific heat of…

Q: coffee-cup calorimeter is filled with 150.0 mL of water at 22.1 °C. A piece of metal at 121.4 °C…

Q: A 15.0-mL sample of benzene at 21.0 °C was cooled to its melting point, 5.5 °C, and then frozen. How…

A: Calculate the mass of benzene from density,

Q: A piece of copper metal (mass = 35.0 g) at 120 °C is placed in a Styrofoam coffee cup containing…

A: We have to calculate the final temperature of water

Q: A 237-g piece of iron, initially at 100.0 °C, is dropped into 244 g of water at 10.0 °C. When the…

A: The amount of heat required to increase the 1oC temperature of 1 g metal is known as the specific…

Q: How many milliliters of water at 31 °C with a density of 1.00 g/mL must be mixed with 95.0 mL (about…

A: Given: Initial temperature of water=31 degree celciusdensity =1.00g/mlvolume of coffee(m2)=95…

Q: A 28.602 g sample of a metal is heated to 99.9°C in a hot water bath until thermal equilibrium is…

A: Let c be the specific heat of the metal Heat lost by the metal = mass x specific heat x temperature…

Q: hot lump of 25.4 g of aluminum at an initial temperature of 83.0 °C is placed in 50.0 mL H2O…

A: This concept is based on principle of calorimetry in this concept heat given by system and heat lose…

Q: A 17.1 g piece of silver was heated to 98.8 °C in boiling water and then dropped into a beaker…

Q: A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O…

A: The given data to you is - mass of Cu = 42.4 g Volume of water = 50 mL Temp of Cu = 64.7 °C Temp of…

Q: A 33.6-g piece of silver initially at 46.5 °C is submerged into 162.4 g of water at 12.3 °C. What is…

A: A hot piece of silver is submerged into cold water, as a result heat will flow from hot silver to…

Q: A piece of titanium metal with a mass of 21.6 g is heated in boiling water to 99.5 °C and then…

A: Since the titanium metal is at a higher temperature, it will lose heat, and water inside the…

Q: A 80.8 g chunk of granite (specific heat: 0.79 J/g°C) is heated to 225.7 °C and dropped into a…

Question

A 47.0-g sample of copper at 99.9 °C is dropped into a beaker containing 157 g of water at 19.0 °C. What is the final temperature when thermal equilibrium is reached? (The specific
heat capacities of liquid water and copper are 4.184 J/g K and 0.385 J/g K, respectively.)
Final temperature =
°C
Save and Exit
E KindleForPC-install.exe
2 Music and mindful.pdf
2 1-s2.0-S01974556.pdf
Show all
5:16 PM
53°F
e Type here to search
10/20/2021
insert
prt sc
144
10
backspac

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

An experiment was conducted to determine the specific heat of platinum. It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC. Based on these experimental results calculate the specific heat (J/g⋅⋅oC) of platinum.
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)
The burning of 28g of vegetable cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5°C to 28.1 Calculate the amount of heat absorbed by the water using the specific heat of water at 4.18 J/gºC.
An experiment was conducted to determine the specific heat of platinum. It was determined that 158.8 Joules of heat were required to increase the temperature of a 50.0 gram sample of platinum from 20.0 oC to 45.5 oC. Based on these experimental results calculate the specific heat (J/g⋅⋅oC) of platinum.
If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?
A hot lump of 36.1 g of aluminum at an initial temperature of 51.1 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
A 87.9 g chunk of limestone (specific heat: 0.22 J/g°C) is heated to 231.9 °C and dropped into a beaker containing 300.0 g of water (specific heat: 4.184 J/g°C) at 20.2 °C.What will be the final temperature of the system after it reaches thermal equilibrium?
A nickel at 30 °C is dropped into a glass of 15.0 g soda at 3.0 °C, if the heat capacity of the nickel is 4.40 J/°C, the heat capacity for the glass is 11.1 J/°C, and the soda has the same specific heat capacity as water (4.184 J/g°C), what is the final temperature of the mixture?
You add 100.0 g of water at 51.7 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools the water to 0.00 °C. When the ice and water mixture reaches thermal equilibrium at 0 °C, how much ice has melted? (The specific heat capacity of liquid water is 4.184 J/g ⋅ K. The enthalpy of fusion of ice at 0 °C is 333 J/g.)
In the laboratory a student finds that it takes 145 Joules to increase the temperature of 14.7 grams of solid silicon from 23.0 to 38.0 degrees Celsius. The specific heat of silicon calculated from her data is J/g°C.
You add 100.0 g of water at 61.0 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools the water to 0.00 °C. When the ice and water mixture reaches thermal equilibrium at 0 °C, how much ice has melted? (The specific heat capacity of liquid water is 4.184 J/g ⋅ K. The enthalpy of fusion of ice at 0 °C is 333 J/g.)