a) Classify the following into intensive and extensive properties.
i) Inernal energy ii) Density
iii) Heat Capacity iv) Temperature
b) Calculate the standard free energy change (`DeltaG^theta`) for the conversion of oxygen to ozone `frac{3}{2}O_(3(g))rightarrowO_(3(g)` at 298 K if the equilibrium constant for the conversion is `2.47xx10^(-29).`
(Given R = 8.314 `JK^-1 mol^-1`)

Classify the following into intensive and extensive properties (i) Internal energy (ii) Density (iii) Heat capacity (iv) Temperature

a) Predict in each of the following whether entropy increses or decreases. i) Sublimation of camphor ii) 4Fe(s)+3O_2(g)rightarrow2Fe_2O_3(g) b) The equilibrium constant for a reaction at 30^oC is 2.5xx10^(-29). What will be the value of DeltaG^o ?

The enthalpy change for the reaction. N_(2(g))+3H_(2(g))rightarrow2NH_(3(g)) is - 91.8 kJ at 298 K.what is Delta U at 298K? ( R=8.314 JK^-1mol^-1 )

The standarid potentiat of a cell. is measured as 1.1V: The,reaction of the cell.is represented-as Zn(s)+Cu^2+(aq) Zn^2+(aq)+Cu(s) i. Calculate the standard free energy change of the reaction. ii Using the calculated value of Delta_r G^circ , find the equilibriam constant of the reaction. iii. If the concentrations of the electrólytes are [Z n^2+]=0.1 ~mol Mitre and [Cu^2+]=0.2 ~mol / litre, calculate the cell 'potentiat.

The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I-(aq) to 2Fe^(2+)(aq) + I_2(s) has E_(cell)^0 = 0.236V at 298 K. Calculate the standard Gibbs energy and equilibrium constant of the cell reaction

The temperature dependence of the rate of a chemical reaction can be accurately explained by Arrhenius equation. With the help of Arrhenius equation, calculate the rate constant for the first order reaction C_2H_5I(g)toC_2H_(4(g))+HI_((G))at700K .Energy of activation (Ea)for the reaction is 209kjmol_(-1) and rate constant at 600K is 1.60xx10^(-5)s^(-1) [Universal gas constant R= 8.314JK^(-1)mol^(-1)]