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.

Q: Why is the standard enthalpy of formation of C0(g), C(s) + ½ 02(g) → CO(g), difficult to measure…

A:

Q: The standard enthalpy of combustion of octane, C8H180 is -5471 kJ-mol-1. The standard enthalpies of…

A: Given,  Standard enthalpy of combustion of C8H18 (l) = ΔH0 = -5471 KJ/mole  Standard enthalpy of…

Q: 50.0 mL of 2.03 M NaOH(aq) is mixed with 50.0 mL of 2.20 M HCl in a Styrofoam calorimeter.…

A:

Q: Using the information given in Table 3, calculate the standard enthalpy for the following reaction.…

A:

Q: When 50.0 mL of 1.24 M of HCI(aq) is combined with 50.0 mL of 1.32 M of NaOH(aq) in a coffee-cup…

A:

Q: For the reaction 2N₂ (9) + O₂(g) → 2N₂O(g) AG=214 kJ and AS = -148.5 J/K at 334 K and 1 atm. This…

A: For the first reaction, we have to find whether the reaction is reactant or product favored and…

Q: (a 7. A 5.00 mol sample of an ideal gas is compressed irreversibly and isothermally at 150.00 K from…

A: Work done in an irreversible and isothermal compression is calculated as: W=-nRTPext1P2-1P1…

Q: A critical reaction in the production of energy to do work or drive chemical reactions in biological…

A:

Q: When 1.0 mol N204(g) is formed from 2.0 mol NO2(g) under constant pressure (1 atm) at 298 K, please…

A: 1.0 mol N204(g) is formed from 2.0 mol NO2(g) Temperature = T = 298 K ΔHf°(NO2,g) = +33.85 kJ/mol…

Q: Calculate the standard enthalpies of combustion at 25ᵒC  (a) C4H8(g) + H2(g) ---> C4H10(g)…

A:

Q: Given the standard enthalpy changes for the following two reactions: (1) Sn(s) + Cl½(g}→SnCl½(s) AH°…

A: Enthalpy (H) is a state function. Hess's Law of constant heat summation: If a chemical reaction…

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.