CHEM 203 Midterm: notes for midterm1.pdf

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18 Aug 2012

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2: temperature dependence of average molecular energies, thermal and bonding energies, quantization, covalent and intermolecular interactions, the 1st law of thermodynamics, systems, surroundings, state functions, processes: Irreversible: heat & work, energy & enthalpy changes, cp & cv, thermochemistry, isothermal & adiabatic calorimetry, hess" law, temperature & heats of reactions, molecular energy changes in reactions, calculation of bond enthalpy & energies, entropy and the 2nd law, entropy, entropy changes, carnot cycle, temperature & entropy, pressure & entropy, s for phase changes, absolute entropies, s for reactions, s for the system, surroundings & the universe, gibb"s energy changes, maximum work, dependence of g on partial pressures & concentrations, equilibrium constants & go, t dependence of k (van"t hoff plots, biophysical applications, bioenergetics & metabolism, coupled processes, diffusion & active transport, hydrophobicity, thermodynamics of protein stability, binding plots and binding constants, multiple equilibria, chemical kinetics, review:

Related Questions

A living plant leaf is an open system that exchanges energy(sunlight and thermal flows) + matter (O₂,CO₂, water vapor, etc.) with the surroundings (theexterior). Even with irreversible processes (energy dissipation) wefind that the net entropy change for the system + surroundings candecrease; i.e. dS < 0. Using equations presented in lecture andyour own critical thinking:
a) Explain how this is possible in terms of d_eS andd_iS.
b) Explain how the Second Law remains valid for this case.

The enzyme-catalyzed hydrolysis of urea(aq) can be represented as follows:

CO(NH₂)₂(aq) + H₂O(l) â CO₂(g) + 2NH₃(aq)

The reaction is carried out in an open solution calorimeter with a calorimeter constant C=485 J/K for the dry calorimeter. When 3.0 g urea is dissolved to make 100 g solution (water + enzyme + pH buffer + urea) allowing hydrolysis to go to completion, the temperature changes from changes from 21.05 to 18.23 ^oC. The specific heat of the solution is 4.25 J/(K.g).

a) Calculate the molar enthalpy of hydrolysis of urea.

b) Using the needed values from the thermodynamic tables, calculate the standard molar entropy change, âS_m^o of the hydrolysis reaction.

c) Again using the needed values from the thermodynamic tables, calculate the standard molar Gibbs energy change, âG_m^o of the reaction.

CHEM 203 Midterm: notes for midterm1.pdf

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