Thermodynamics ...

If $$\Delta G$$ for a reaction is negative, the change is:

Determine $$ \Delta U^o $$ at 300 K for the following reaction using the listed enthalpies of reaction :
$$ 4CO(g)+8H_{ 2 }(g)\rightarrow 3CH_{ 4 }(g)+CO_{ 2 }(g)+2H_{ 2 }O(I) $$
$$ C (graphite)+1/2O_2(g) \rightarrow CO(g); \Delta H^o_1 = -110.5 kJ $$
$$ CO(g) +1/2 O_2(g) \rightarrow   CO_2(g); \Delta H^o_2 = -282.9 kJ $$
$$ H_2(g) + 1/2 O_2(g) \rightarrow H_2O(I); \Delta H^o_3 = -285.8 kJ $$
$$ C(graphite)+2H_2(g) \rightarrow   CH_4(g); \Delta H^o_4 = -74.8 kJ $$

The Normal boiling point of a liquid 'X' is $$400$$ K. Which of the following statement is true about the process $$X(l) \rightarrow X(g)$$?

For hydrogenation of ethene into ethane  as per following chemical reaction $$CH_2=CH_2+H_2 \xrightarrow[]{Pd} CH_3-CH_3$$
The $$\Delta H_{reaction}$$ is written as
Calculate $$\Delta H_{reaction}$$ for

For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter $$\Delta U$$ and w correspond to 

An ideal gas is taken through a cyclic thermo dynamical process through four steps. The amounts of heat involved in steps are
$$Q_1 = 5960 J, Q_2 = -5585 J, Q_3 = -2980 J, Q_4 = 3645 J$$; respectively, the corresponding works involved are $$W_1 = 2200 , W_2 = -825 J, W_3 = -1100 J$$ and $$W_4$$ respectively. Find the value of $$W_4$$ and efficiency of the cycle

Assertion : In Free expansion, $$\Delta U = 0$$
Reason : No work is done in free expansion

At $$5\times 10^{5}$$  bar pressure density of diamond and  graphite are  3 g/cc adn 2 g/ cc respectively.   at certain temperature 'T'    Find the  value of  $$\Delta U-\Delta H$$   for the conversion of 1 mole of  graphite to 1 mole of diamond at termperature 'T'

$$5$$ mole of ideal gas at $$100K$$ ($${C}_{v,m}=28J/mol/K$$). It is heated upto $$200K$$. Calculate $$\Delta U$$ and $$\Delta (PV)$$ for the process. ($$R=8J/mol-K$$)

A diatomic ideal gas is expanded at constant at pressure. If work done by the system is $$10 \,J$$ then calculate heat absorbed.