6.22 Calculate the entropy change in surroundings when 1.00 mol of is formed under standard conditions.
6.21 Comment on the thermodynamic stability of NO(g), given
6.20 The equilibrium constant for a reaction is 10. What will be the value of
6.19 For the reaction
Calculate for the reaction, and predict whether the reaction may occur spontaneously.
6.18 For the reaction, , what are the signs of ?
6.17 For the reaction at 298 K,
2A + B C
At what temperature will the reaction become spontaneous considering and to be constant over the temperature range.
6.16 For an isolated system, , what will be ?
6.15 Calculate the enthalpy change for the process and calculate bond enthalpy of in
6.14 Calculate the standard enthalpy of formation of CH3OH(l) from the following data:
6.13 Given .What is the standard enthalpy of formation of gas?
6.12 Enthalpies of formation of are –110, – 393, 81 and 9.7 respectively. Find the value of for the reaction:
6.11 Enthalpy of combustion of carbon to is Calculate the heat released upon formation of 35.2 g of from carbon and dioxygen gas.
6.10 Calculate the enthalpy change on freezing of 1.0 mol of water at to ice at .
6.9 Calculate the number of kJ of heat necessary to raise the temperature of 60.0 g of aluminium from to . Molar heat capacity of Al is
6.8 The reaction of cyanamide, (s), with dioxygen was carried out in a bomb calorimeter, and was found to be at 298 K. Calculate enthalpy change for the reaction at 298 K.
6.7 In a process, 701 J of heat is absorbed by a system and 394 J of work is done by the system. What is the change in internal energy for the process?
6.6 A reaction, A + B C + D + q is found to have a positive entropy change. The reaction will be
(i) possible at high temperature
(ii) possible only at low temperature
(iii) not possible at any temperature
(v) possible at any temperature
6.5 The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, and respectively. Enthalpy of formation of will be
6.4 of combustion of methane is . The value of is
(iv) = 0
6.3 The enthalpies of all elements in their standard states are:
(iii) < 0
(iv) different for each element