If 50.5 g of KBr are dissolved in 400.0 g of water at 25.0 °C in an insulated container, a temperature change is observed. The AH of solution of KBr is 19.9 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?

If 50.5 g of KBr are dissolved in 400.0 g of water at 25.0 °C in an insulated container, a temperature change is observed. The AH of solution of KBr is 19.9 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?

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: 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: The enthalpy of solution (AH) of KOH is -57.6 kJ/mol. If 2.91 g is dissolved in enough water to make…

A: Given: Volume of solution = 150.0 mLDensity of solution = 1.02 g/mL.Enthalpy of solution of KOH =…

Q: When 75.71 grams of fictional compound X is added to water to make 367.7 grams of solution, the…

Q: If 55.5 g of KBr are dissolved in 400.0 g of water at 25.0 °C in an insulated container, a…

Q: Macmillan Learning Revell SECOND EDITION q= A chemist dissolved an 12.7-g sample of KOH in 100.0…

A: Given, Mass of the sample, m1 = 12.7 g Mass of water, m2 = 100 g Specific heat of water, C =…

Q: If 27.5 g of MgCl₂ are dissolved 500.0 g of water at 20.0 °C in an insulated container, a…

A: Given that, The mass of the MgCl2 is 27.5 g. The mass of the water is 500.0 g. So, the total mass of…

Q: How many milliliters of water at 21 °C with a density of 1.00 g/mL must be mixed with 220 mL of…

Q: When 15.53 grams of fictional compound X is added to water to make 344.5 grams of solution, the…

Q: 3. When 2.0 g of NaOH is the heat of dissolution are dissolved in 49.0 g of water, the temperature…

A: 3.) First we need to calculate the heat using the formula Q = mC∆T Then we need to calculate moles…

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: A calorimeter contains 365 g of water at 30.0 °C. A 29.3-g sample of ice (at -11.0 °C) is added to…

A: We have to calculate the final temperature of water

Q: hen 92.00 grams of fictional compound X is added to water to make 531.0 grams of solution, the…

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: A 0.562 g sample of KCl is added to 35.8 g of water in a calorimeter. If the temperature decreases…

A: The heat capacity of the resulting solution is 4.18 J/goC, which states that 4.18 J of energy will…

Q: When 98.88 grams of fictional compound X is added to water to make 386.9 grams of solution, the…

A: Given mass of solution = 386.9 g mass of X = 98.88 g molar mass of X = 125.14 g/mol specific heat =…

Q: What is the final temperature when a 5.0 g sample of brass initially at 25 oC absorbs 75 J of heat?…

A: Equation for finding the heat absorbed by brass is as follows. Q=mc∆TQ=heat absorbed by brassm=mass…

Q: 20.9 g of sodium nitrate is added to a coffee cup calorimeter. The calorimeter initially contained…

Q: neat re

Q: A calorimeter contains 2.50 kg g of water at 37.0 °C. A 225-g sample of ice (at -20.0 °C) is added…

Q: If 80.5 g of KBr are dissolved in 400.0 g of water at 25.0 °C in an insulated container, a…

Q: Determine the final temperature of a 32.3 mL salt solution initially at 21.05ºC when 1.93 kJ of heat…

A: Volume of solution(V) = 32.3 mL Density of solution(d) = 1.235 g/mL Mass = V × d = 32.3 × 1.235 =…

Q: student is asked to determine the heat of solution in J/g for the compound ammonium nitrate…

Q: How much heat (in Joules) is gained by 447 grams of water that is warmed from 25.0 J °C to 54.0°C?…

A: The amount of heat absorbed (or released) by fixed amount of a substance to change its temperature…

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 solution is made by mixing 197.3 g of ethanol initially at 10.5°C with 250.0 g of water initially…

A: We know that, according to the law of conservation of heat energy, energy gained or loss by the…

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: When a 43.0 g sample of metal at 100.0 oC is added to 38.0 g of water at 23.72 oC, the final…

Q: sample of water with a mass of 726.2 g undergoes a temperature change from 58.32oC to 40.50 oC. What…

A: Given, mass, m = 726.2 g Specific heat of water (l), S = 4.184 J/g. oC Temperature changes from T1…

Q: A solution is made by mixing 260.0 mL of ethanol initially at 15.5 °C with 260.0 mL of water…

A: Given volume ethanol =260.0 mLinitial temperature of ethanol =15.5 °Cdensity of ethanol =0.789…

Q: What is the heat of solution for compound X

Q: A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric g…

Q: When 37.00 grams of fictional compound X is added to water to make 526.0 grams of solution, the…

A: Temperature flow from higher temperature to the low temperature. q= mc∆T Heat capacity of water=…

Q: Ices] A 21.0 g sample of pure iron at 85 °C is dropped into 66 g of water at 20. °C. What is the…

A: The given problem can be solved by using the formula given below as; mironCiron∆T = mwaterCwater∆T…

Q: When 2.105 g of NH4NO3 (molar mass is 80.05 g/mL) is added to 100.0 mL of water at 25.05C, the final…

A: To calculate the molar heat of the solution of NH4NO3 in KJ/mol Given that: Mass of solute = 2.105…

Question

esc
W
Н
H: | PF | Pr | HGwGwGta WHGW (3 il MOC2 |O|A|
app.101edu.co
Week 4 Lab 3....docx
If 50.5 g of KBr are dissolved in 400.0 g of water at 25.0 °C in an
insulated container, a temperature change is observed. The AH of
solution of KBr is 19.9 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?
1
F1
Q
2
F2
W
3
20
F3
W
E
की व
4
000
DOO
F4
R
do L
%
5
F5
Question 16 of 28
MacBook Air
T
6
F6
&
Y
7
F7
U
DII
8
FB

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

Final answer

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Follow-up Questions

Read through expert solutions to related follow-up questions below.

Follow-up Question

Solution

by Bartleby Expert

SEE SOLUTION

Similar questions

A particular sample of cold graphite at 10.20 °C was added to 988.5 g of water at 25.31 °C in a constant pressure calorimeter. If the final temperature of the graphite and water was 25.17 °C, what was the mass of the graphite sample? Assume no heat was lost to the surroundings. The specific heat for water is 4.184 J/g•°C and the specific heat for this graphite is 0.7069 J/g•°C.
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.
When 40.00 grams of fictional compound X is added to water to make 236.0 grams of solution, the temperature increases from 19.05 °C to 63.46 °C. What is the heat of solution for compound X (in kJ/mol) given that the molar mass of compound X is 73.87 g/mol. Assume the specific heat capacity of the solution is 4.18 J/g°C.
How much heat would have to be absorbed by 2000 g of water to change its temperature from 20°C to 50°C? Use the value 4.2 J/mol °C for the specific heat of water.
Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
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?
For cyclohexane, the ∆H° of vaporization is 33.10 kJ/mol and the ∆S° of vaporization is 111.80 J/mol･K. At 1.00 atm and 201 K, what is the ∆G° of vaporization for cyclohexane, in kJ/mol?
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).
A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water initially at 22.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C ?f= ∘C
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?