Cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as where ADP represents adenosine diphosphate. For this reaction, `"deltaG^(@)` is 30 kJ/mol and `delta H^0` is -30 kJ/mol at `27^(@)C`. Calculate the entropy change.

The standard potential of a cell using the reaction is 1.12 . The heat of the reaction is -504.2kJ mol ^(-1) at 25^(@)C . Calculate the entropy change.

The enthalpy change for the transition of liquid water to steam Delta_("vap")H is 40.8 kJ mol^(-1) at 100^@C . Calculate the entropy change (Delta_("vap")S) for the process.

The hydrolysis of Adenosine triphosphate [ATP] to give adenosine diphosphate [ADP] is represented by ATP harr ADP. This reaction is exothermic zero[K] . The entropy change for the reaction is 982 J/K at 310 K . The free energy for the reaction is:

If the enthalpy change for the transition of liquid water to steam is 30 kJ mol^(-1)" at " 27^@C the entropy change for the process would be

The emf of the cell reaction Zn(s) +Cu^(2+) (aq) rarr Zn^(2+) (aQ) +Cu(s) is 1.1V . Calculate the free enegry change for the reaction. If the enthalpy of the reaction is -216.7 kJ mol^(-1) , calculate the entropy change for the reaction.

For an endothermic reaction, where Delta H represents the enthalpy of reaction in kJ mol^(-1) , the minimum value for the energy of activation will be

For a certain reaction the change in enthalpy and change in entropy are 40.63 kJ mol^(-1) and 100 JK^(-1) .What is the value of Delta G at 27^(@)C and indicate whether the reaction is possible or not ?

The standard free energy change of a reaction is DeltaG^(@)=-115kJ//mol^(-1) at 298 K. Calculate the value of log_(10)K_(p) (R=8.314JK^(-1)mol^(-1))

Fuel cells : Fuel cells are galvanic cells in which the chemical energy of fuel cell is directly converted into electrical energy. A type of fuel cell is a hydrogen - oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst ( platinum, silver, or metal oxide ). The electrodes are placed in aqueous solution of NaOH . Oxygen and hydrogen are continuously fed into the cell. Hydrogen gets oxidized to H^(o+) which is neutralized by overset(c-)(O)H, i.e., anodic reaction. At cathode, O_(2) gets reduced to overset(c-)(O)H Hence, the net reaction is The overall reaction has DeltaH=-285.6 kJ mol^(-1) and DeltaG=-237.4 kJ mol^(-1) at 25^(@)C What is the value of DeltaS^(c-) for the fuel cell at 25^(@)C ?

As per second law of thermodynamics a process taken place spontaneously if and only if the entropy of the universe increases due to the process. Change in entropy is given by Delta S = (Q_(rev))/(T) What is the change in entropy of the universe due to the following reaction occuring at 27^(@)C ? A + 2B rarr C + 2D, Delta H = +1.8 kJ mol^(-1) Molar entropy values of A, B, C and D are 1,2,3 and 4 JK^(-1) mol^(-1) respectively.