A calorimeter contains 33.0 mL of water at 14.5 °C. When 2.10 g of X (a substance with a molar mass of 62.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(1)→X(aq) and the temperature of the solution increases to 25.0 °C. Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g°C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. View Available Hint(s) Consider the reaction C12H22 O11 (s) + 1202 (g)→12CO2 (g) +11H₂O(1) in which 10.0 g of sucrose, C12 H22 O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
A calorimeter contains 33.0 mL of water at 14.5 °C. When 2.10 g of X (a substance with a molar mass of 62.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(1)→X(aq) and the temperature of the solution increases to 25.0 °C. Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g°C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings. Express the change in enthalpy in kilojoules per mole to three significant figures. View Available Hint(s) Consider the reaction C12H22 O11 (s) + 1202 (g)→12CO2 (g) +11H₂O(1) in which 10.0 g of sucrose, C12 H22 O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
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![A calorimeter contains 33.0 mL of water at 14.5 °C. When 2.10 g of X (a substance with a molar mass of 62.0 g/mol) is added, it dissolves via the reaction
X(s)+H2O(1)→X(aq)
and the temperature of the solution increases to 25.0 °C.
Calculate the enthalpy change, AH, for this reaction per mole of X.
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- °C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter
itself, nor to the surroundings.
Express the change in enthalpy in kilojoules per mole to three significant figures.
► View Available Hint(s)
Consider the reaction
C12H22 O11 (s) + 1202 (g)→12CO₂ (g) + 11H₂O(1)
in which 10.0 g of sucrose, C12H22 O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be
22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose.
Express the change in internal energy in kilojoules per mole to three significant figures.
► View Available Hint(s)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F41accc56-b3f8-400a-945c-6e1aea95d85d%2F7ca5fe33-4c17-414c-9a7d-f8bffad18376%2Fids21ln_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A calorimeter contains 33.0 mL of water at 14.5 °C. When 2.10 g of X (a substance with a molar mass of 62.0 g/mol) is added, it dissolves via the reaction
X(s)+H2O(1)→X(aq)
and the temperature of the solution increases to 25.0 °C.
Calculate the enthalpy change, AH, for this reaction per mole of X.
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g- °C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter
itself, nor to the surroundings.
Express the change in enthalpy in kilojoules per mole to three significant figures.
► View Available Hint(s)
Consider the reaction
C12H22 O11 (s) + 1202 (g)→12CO₂ (g) + 11H₂O(1)
in which 10.0 g of sucrose, C12H22 O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be
22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose.
Express the change in internal energy in kilojoules per mole to three significant figures.
► View Available Hint(s)
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