Thermodynamics ...

The statement "The change of enthalpy of a chemical reaction is same whether the reaction takes place in one or several steps" is:

1 mole of an ideal gas STP is subjected to a reversible adiabatic expansion to double its volume. The change in internal energy $$(\gamma = 1.4)$$ 

For the reaction at $$\ { 25 }^{ o }C,{ X }_{ 2 }{ O }_{ 4(l) }\longrightarrow 2X{ O }_{ 2(g) }\quad $$
$$\Delta H=2.1kcal$$ and $$\Delta S=20cal\quad { K }^{ -1 }$$. 

Internal energy of an ideal gas depends upon

Three stars A, B, C have surface temperatures $$T_A$$, $$T_B$$ and $$T_C$$. A appears bluish, B appears reddish and C appears yellowish. We can conclude that:

1 kg of water is heated from 40 C to 70 C, If its volume remains constant, then the change in internal energy is (specific heat of water = 4148 J$${ kg }^{ -1 }{ K }^{ -1 })$$

An electric heater supplies heat to a system at a rate of 120 W. If system performs work at a rate of 80 J $${ s }^{ -1 }$$, the rate of increase in internal energy is :

An ideal gas undergoing a change of state from A  to  B  through   four  different  paths  I,   II   ,III  and   IV  as  shown  in  the  P-V  diagram  that   lead  to  the  same  change of state, then the change in internal energy is

For the combustion of $$CH_4$$ at 1 atm pressure & 300 K, which of the following options is correct?
$$2M + O_2 \xrightarrow  2MO$$
$$\Delta G_{1000 ^{\circ}C} = -921 kJ/mol$$
$$\Delta G_{1900 ^{\circ}C} = -300 kJ/mol$$
$$2C + O_2 \xrightarrow 2CO$$
$$\Delta G _{1000 ^{\circ}C} = -432 kJ/mol$$
$$\Delta G_{1900 ^{\circ}C} = -624 kJ/mol$$
$$MO + C \xrightarrow{\Delta} M + CO \uparrow$$
This reaction is feasible at temperature:

Which of the following parameters does not charaterize the thermodynamic state of matter?