The enthalpy of the following reaction at 1.00 atm and 298.15K is -56.9kJmol-1 H* (ag) + OH (ag) →H,Oµ, When 2mol of an aqueous acid (H* (aq) reacts with 2mol of an aqueous base (OH(a9) in a thermally isolated constant pressure calorimeter initially at 298.15K, the temperature was observed to increase to 304.35K. In the exact same calorimeter, the hydrolysis of 1.7mol of aqueous adenosine 5'- triphosphate (ATP) caused an increase in temperature from 298.15K to 300.95K. (a) What is the enthalpy of hydrolysis per mol of ATP? (b) The hydrolysis of ATP is the primary mechanism by which the energy required by the human body is released. Assuming that the human body can use all of the released energy from ATP hydrolysis, how many grams of ATP is necessary to undergo hydrolysis per day to provide the average human daily energy requirement of 2000kcals (Molar mass of ATP =507.181gmol-1), assuming no other source of energy.

The enthalpy of the following reaction at 1.00 atm and 298.15K is -56.9kJmol-1 H* (ag) + OH (ag) →H,Oµ, When 2mol of an aqueous acid (H* (aq) reacts with 2mol of an aqueous base (OH(a9) in a thermally isolated constant pressure calorimeter initially at 298.15K, the temperature was observed to increase to 304.35K. In the exact same calorimeter, the hydrolysis of 1.7mol of aqueous adenosine 5'- triphosphate (ATP) caused an increase in temperature from 298.15K to 300.95K. (a) What is the enthalpy of hydrolysis per mol of ATP? (b) The hydrolysis of ATP is the primary mechanism by which the energy required by the human body is released. Assuming that the human body can use all of the released energy from ATP hydrolysis, how many grams of ATP is necessary to undergo hydrolysis per day to provide the average human daily energy requirement of 2000kcals (Molar mass of ATP =507.181gmol-1), assuming no other source of energy.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 121QRT

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

The enthalpy of the following reaction at 1.00 atm and 298.15K is -56.9kJmol-1
H* (ag) + OH (ag) →H,Oµ,
When 2mol of an aqueous acid (H* (aq) reacts with 2mol of an aqueous base (OH(a9)
in a thermally isolated constant pressure calorimeter initially at 298.15K, the
temperature was observed to increase to 304.35K.
In the exact same calorimeter, the hydrolysis of 1.7mol of aqueous adenosine 5'-
triphosphate (ATP) caused an increase in temperature from 298.15K to 300.95K.
(a) What is the enthalpy of hydrolysis per mol of ATP?
(b) The hydrolysis of ATP is the primary mechanism by which the energy required
by the human body is released. Assuming that the human body can use all of the
released energy from ATP hydrolysis, how many grams of ATP is necessary to
undergo hydrolysis per day to provide the average human daily energy
requirement of 2000kcals (Molar mass of ATP =507.181gmol-1), assuming no
other source of energy.

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