One mole of naphthalene (`C_10H_8`) is burnt in oxygen at constant volume to give `CO_2` and water at `25^@C` The heat evolved is found to be -5138.8 KJ `mol^(-1)` Calculate the heat of reaction at constant pressure.

The standard enthalpy of formation of ammonia is -42.19 kJ. Calculate the heat of the following reaction at constant volume. N_2(g) + 3H_2(g) rarr 2NH_3(g)

The ratio of specific heat of a agas at constatnt pressure to that constatnt volume is gamma . The change in internal energy of one mole of a gas when volume changes from V to 2V at constant pressure P is

Henry's law constant for CO_2 in water is 1.67xx10^8 Pa at 298 K. Calculate the quantity of CO_2 in 500mL of soda water when packed under 2.5 atm CO_2 pressue at 298K.

For the conversion of 1 mole of SO_2(g) to SO_3(g) the heat of reaction at constant volume ( Delta U^@ ) at 298K is -97.027 KJ Calculate the enthalpy change ( Delta H^@ )

Answer the following questions based on the P-T phase diagram of CO_2 : Describe qualitatively the changes in a given mass of solid CO2 at 10 atm pressure and temperature 65^-@C as it is heated up to room temperature at constant pressure

For a decomposition reaction, the values of rate constants at two different temperatures are given below: K_1 = 2.15xx10^-8 Lmol^-1s^-1 at 650k K_2 = 2.39xx10^-7 Lmol^-1s^-1 at 700k Calculate the value of activation energy for the reaction (R = 8.314 JK^-1 mol^-1 )

Two elements A and B form compounds having formula AB_2 and AB_4 . When dissolved in 20 g of benzene (C_6H_6) , 1 g of AB_2 lowers the freezing point by 2.3 K whereas 1.0 g of AB_4 lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^-1 . Calculate atomic masses of A and B.

The reaction N_2O_5 rarr 2NO_2 + 1/2O_2 is first order in N_2O_5 . Its rate constant is 6.2xx10^-6s^-1 . If in the beginning [N_2O_5] is 1.25 mol L^-1 , Calculate the rate reaction in the beginning.

The rate constant of reaction is 1.5xx10^7s^-1 at 50^@C and 4.5xx10^7s^-1 at 100^@C . Calculate the value of activation energy for the energy for the reaction (R = 8.314 Jk^-1 mol^-1)