A 14.7-g sample of iron pellets (specific heat capacity 0.460 J/°C.g) and a 13.4-g sample of gold pellets (specific heat capacity 0.126 J/ °C g) were heated to 195°C. The mixture of hot metal is dropped into 125 g of ethylene glycol (specific heat capacity 2.43 J/°C g) at 21.3°C. Assuming no heat loss to the surroundings, calculate the final temperature of the metal and ethylene glycol mixture.

A 14.7-g sample of iron pellets (specific heat capacity 0.460 J/°C.g) and a 13.4-g sample of gold pellets (specific heat capacity 0.126 J/ °C g) were heated to 195°C. The mixture of hot metal is dropped into 125 g of ethylene glycol (specific heat capacity 2.43 J/°C g) at 21.3°C. Assuming no heat loss to the surroundings, calculate the final temperature of the metal and ethylene glycol mixture.

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 498.00 sample of an unknown metal at 92.15°C is placed in a calorimeter containing 185.00 mL of…

A: At the thermal equilibrium, the heat lost by the metal is equal to the gained by the water.…

Q: 1. A piece of titanium metal (mass 452.398 g) is placed in boiling water (100.00 °C). After 20…

A: (1) When the Titanium metal is placed in boiling water, it comes to the thermal equilibrium with the…

Q: The table lists the specific heat capacities of select substances. Substance Specific heat capacity…

A: The amount of heat required to increase the temperature of the 1 g of the substance by 1 degree is…

Q: Two 66-g ice cubes at 0 °C are dropped into 5.00 x 102 mL of tea to make iced tea. The tea was…

A: The mass of tea (m) is calculated as follows:

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: If 40.0 g of hot water at 80.0oC is added to 60.0 g of cold water at 20.0oC, what is the final…

A: The final temperature is 44 oC

Q: By a hot summer day, you want to serve some refreshments to your friends. To each glass, if you pore…

A: Given: Volume of team = 200.0 mL. Initial temperature of tea = 20.0 oC Mass of each ice cube = 10.0…

Q: a) We place 125.0 g of a metal at 5.00°C in 350.0 g of water at 100.00°C. The water is in a beaker…

A: Problem a) CalorimetryUnderstanding the ProblemA hot metal is placed in cold water in a beaker.We…

Q: What is the specific heat capacity of an unknown metal if 75.00 g of the metal absorbs 418.6J of…

A: Calculation of heat capacity: The amount of heat required to increase the temperature of one gram of…

Q: A 45.2-g iron rod, initially at 12.9 oC is submerged into 55.2 g of water at an unknown initial…

A: Given data: Mass of iron rod = mFe = 45.2-g Initial temperature of iron rod = Ti(Fe)= 12.9°C Mass of…

Q: A 5.00-g sample of aluminum pellets (specific heat capacity= 0.89 J/°C-g) and a 15.00-g sample of…

Q: 1. PBR3 IR (cm-1): 3480 (broad), 2800-3000, 1708 (strong) HO MS (m/z): 86 (molecular ion) 2. но 3.…

A: There is error in your 5th step. You can check out 2 step to get your mistake.

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: substance initially at 181.6 °C is placed in 35.0 mL of water initially at 25.0 °C and the system is…

Q: A 50 gram sample of iron (with a heat capacity of 0.450 J/g ºC) is heated to 100.0 ºC. It is then…

A: Answer :- Heat absorbed by the calorimeter = 1111 J…

Q: A 8.50-g sample of aluminum pellets (specific heat capacity=0.89 C-g) and a 22.50-g sample of iron…

A: we have to calculate the final temperature

Q: A hot lump of 25.225.2 g of iron at an initial temperature of 65.0 °C65.0 °C is placed in 50.0 mL…

A: Given,Mass of hot iron lump = 25.2 gInitial temperature of hot iron lump = 65.0 °CVolume of water…

Q: A 2.62E1 g sample of aluminum at 1.008E2 °C is added to 1.002E2 g of water at 2.22E1 °C in a…

A: For a chemical reaction or physical process to occur a certain amount of energy should be furnished…

Q: 50.0 mL of hot water (49.6 oC) is added to 50.0 mL of cold water (24.7 oC). Upon mixing the water…

A: Given: For hot water Volume, V= 50.0ml So, mass m1= d x V = 1 x 50.0 = 50g Temperature T1= 49.6oC…

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 60.86-g stainless steel ball bearing at 115.81°C is placed in a constant-pressure calorimeter…

Q: A hot 111.6 g lump of an unknown substance initially at Substance Specific heat (J/(g.°C)) 150.0 °C…

A: By help of Following formula we can calculate the specific heat of the unknown Substance - M1 C1…

Q: 1 Calculate the amount of heat needed to raise the temperature of 50.0 g of iron from 21.0°C to…

A: As per bartleyby guidelines i answered only first question so please don't mind and post other…

Q: In the lab, an experimenter mixes 75.0 g of water (initially at 30o C) with 83.8 g of a solid metal…

A: To determine the specific heat capacity of any particular metallic substance, calculate the energy…

Q: Draw the major organic product of the reaction shown below. OH + HBr

Q: A 328.00 sample of an unknown metal at 87.78°C is placed in a calorimeter containing 136.00 mL of…

A: The principle of the calorimeter is the heat energy transferred between the water in the calorimeter…

Q: What is the heat of solution for compound X

Q: A hot lump of 47.547.5 g of iron at an initial temperature of 51.5 °C51.5 °C is placed in 50.0 mL…

Q: A piece of metal with a mass of 59.047 g was heated to 98.0°C and then put into 100.0g of water…

A: Given: Mass of the metal = 59.047 g The initial temperature of the metal = 98.0 oC The mass of water…

Q: A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a…

A: Given : Mass of water = 39.9 g Mass of metal = 43.5 g Initial temperature of water = 25.1 oC Final…

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…

Question

A 14.7-g sample of iron pellets (specific heat capacity 0.460 J/°C.g)
and a 13.4-g sample of gold pellets (specific heat capacity 0.126 J/
°C g) were heated to 195°C. The mixture of hot metal is dropped
into 125 g of ethylene glycol (specific heat capacity 2.43 J/°C g) at
21.3°C. Assuming no heat loss to the surroundings, calculate the
final temperature of the metal and ethylene glycol mixture.
1
4
7
+/-
°C
2 3
5 6
8
9
0
X
C
x 100
C
G

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

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 46.9-g iron rod, initially at 18.6 oC is submerged into 50.4 g of water at an unknown initial temperature. The final temperature of the mixture upon reaching thermal equilibrium is 69.6 oC. What is the initial temperature of the water (in oC)? The specific heat capacity of iron is 0.449 J/g.oC The specific heat capacity of water is 4.184 J/g.oC
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 molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
51