
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question

Transcribed Image Text:Exercise 6.123
An ice cube of mass 9.0 \({\rm g}\) at temperature
O^\circ C) is added to a cup of coffee, whose
temperature is 85 \({\rm Acirc C}\) and which
contains 110 \{\rm g}) of liquid. Assume the
specific heat capacity of the coffee is the same as
that of water. The heat of fusion of ice (the heat
associated with ice melting) is 6.0N
Part A
Find the temperature of the coffee after the ice melts.
Express your answer using two significant figures.
?
DAL
ATI) =
1(^circ {\rm CH
Submit
Request Answer
Return toAssignment
IProvide Feedback
om/myct/itemView?assignmentProblemID=174388868
(
acer
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
Trending nowThis is a popular solution!
Step by stepSolved in 4 steps

Knowledge Booster
Similar questions
- A piece of metal weighing 8.00 g at a temperature of 46.0 oCo was placed in a calorimeter in 38.10 mL of water at 24.3 oC. The final equilibrium temperature was found to be 25.7 oC . What is the specific heat of the metal?arrow_forwardA quantity of 2.00×102 mL of 0.786 M HCl is mixed with 2.00×102 mL of 0.393 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.76°C. For the process below, the heat of neutralization is −56.2 kJ/mol. What is the final temperature of the mixed solutions? H+(aq) + OH−(aq)→H2O(l) _____°Carrow_forwardCalculate the standard enthalpy of formation for C3H6O (l) from its combustion using the following data: Enthalpy of this combustion is -1793 kJ ( you must write a balanced reaction first).arrow_forward
- 12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. calorimeter itself.)arrow_forwardCalcium acetate, Ca(CH3COO)2 has a molar mass of 158.17 g/mol. In a constant pressure calorimeter, 44.2 g of Ca(CH3COO)2 is dissolved in 861g of water at 25.00 °C. The heat produced by the solution was determined to be 15kJ. What is the final temperature of the solution? q= - msAT SH20 = 4.184 29.0 °C O 18.4 °C O 64.6 °C O 33.8 °C O 3.96 °C O 21.0 °Carrow_forwardWhich of the following reactions occuring at 25° C defines the standard enthalpy of formation (TriangleHf) of liquid water? - 2 H (g) + O (g) -> H2O (l) - H2O(g) + O (g) -> H2O (l) - H2 (g) + ½O2 (g) -> H2O (l) - 2 H2 (g) + O2 (g) -> 2 H2O (l)arrow_forward
- The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = auarrow_forwardHw.77.arrow_forward15 g of solid MgCl2 is mixed with 30 g of water in a calorimeter that absorbs no heat. Which equation calculates the temperature change? Question 16 options: (15 g / 53.49 g mol–1 × –159850 J mol–1) / (30 g × 4.184 J g–1 °C–1) (15 g / 53.49 g mol–1 × 159850 J mol–1) / (30 g × 4.184 J g–1 °C–1) –(15 g / 53.49 g mol–1 × –159850 J mol–1) / (45 g × 4.184 J g–1 °C–1)arrow_forward
- What is the specific heat capacity of a substance of mass 159.5 g that increases in temperature from 22.2 °C to 25.2 °C after absorbing 1.15 kJ of energy in the form of heat? Express your answer in J g-1 °C-1. Do not try to identify the substance.arrow_forwardThe enthalpy of combustion of methane gas, CH4(g), is about -9.0*102 kJ/mol. When methanegas reacts with O2(g), the products are carbon dioxide CO2(g) and water H2O(l). How much heatis released during the combustion of methane gas when 4.0 mols of O2(g) are consumed. Express your answer in kJ.A. 3.0*102 kJB. 6.0*102 kJC. 9.0*102 kJD. 12*102 kJE. 18*102 kJarrow_forwardA 3.450 g of propane (molar mass = 44.11 g/mol) was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 24.000 degrees celsius and its total heat capacity was 76.65 kJ * C^-1. The reaction raised the temperature of the calorimeter to 28.965 degrees celsius. a. What is the heat exchangged by the reaction in kilojoules, qrxn? b. Calculate the deltaE rxn for the combustion of propane in kilojoules per mole c. Work in this reaction is done on the system, done on the surroundings, or equal to zero? Why?arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY

Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning

Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education

Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning

Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning

Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY