Thermodynamics ...

Select correct statement.

An ideal monoatomic gas undergoes a process in which its internal energy U and density $$\rho$$ vary as $$U\rho\, =\, constant.$$ The ratio of change in internal energy and the work done by the gas is

Heat of reaction for the reaction is:

The dissolution of 1 mole of NaOH(s) in $$100 \: mole \: of \: H_2O(l)$$ give rise to evolution of heat as -42.34 kJ. However, if1 mole of NaOH(s) is dissolved in $$1000 \:mole \:of \:H_2O(l)$$ the heat given out is 42.76 kJ. 

The heat measured for a reaction in bomb calorimeter is :

1 gram sample of $$NH_4NO_3$$ is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by 6.12 K. The heat capacity of the system is 1.23 kJ/g-deg. What is the molar heat of decomposition for $$NH_4NO_3$$?

The $$\Delta_f H^{\circ}$$ for $$CO_2 (g), \: CO(g) \: and \: H_2O(g)$$ are $$-393.5, -110.5$$ and $$-241.8 \: kJ \: mol^{-1}$$ respectively. The standard enthalpy change (in kJ) for the reaction is:

The commercial production of water gas utilize the reaction under standard conditions:

The enthalpies of formation of $$N_2O$$ and $$NO$$ are $$28$$ and $$90\ kJ mol^{-1}$$ respectively. The enthalpy of the reaction, $$2N_2O(g) +O_2(g)\longrightarrow 4NO(g)$$ is equal to :

Which of the following has the same value as $$\Delta_f H^{ \ominus }$$ , $$CO$$
a. $$\frac { 1 }{ 2 } \Delta_f H^{ \ominus } (CO_2)$$
b. $$\frac { 1 }{ 2 } \Delta_c H^{ \ominus } (graphite)$$
c. $$\Delta_f H^{ \ominus } (CO_2) - \Delta_f H^{ \ominus } (graphite)$$
d. $$\Delta_c H^{ \ominus } (graphite) - \Delta _c H^{ \ominus } (CO)?$$