Thermodynamics ...

The value of $$\Delta G$$ for the process $${ H }_{ 2 }O\left( s \right) \rightarrow { H }_{ 2 }O\left( l \right)$$  at 1 atm and 260 K is:

Statement I: In adsorption process, the value of $$\Delta H$$ is always negative.
Statement II: During adsorption surface area of adsorbent decreases.
Which of the above statement is/are true? Choose the correct option.

For the reversible isothermal expansion of one mole of an ideal gas at $$300$$ $$K$$, from a volume of $$10 L$$ to $$20 L$$, $$\Delta H$$ is :

For the process $${ H }_{ 2 }O(1,1bar,373.15k)\rightarrow { H }_{ 2 }O(g,1bar,373.15k)$$, the correct set of thermodynamic parameters is:

For reversible isothermal expansion of one mole of an ideal gas at $$300 K$$, from a volume of $$10 L$$ to $$20 L$$, $$\Delta H$$ is :

For the hypothetical reaction: $${ A }_{ 2 }\left( g \right) +{ B }_{ 2 }\left( g \right) \rightleftharpoons 2AB\left( g \right)$$

Two reactions are given below:$${ CO }_{ \left( g \right)  }+\dfrac { 1 }{ 2 } { O }_{ 2\left( g \right)  }\rightarrow { CO }_{ 2\left( g \right)  }$$$${ { Ag }_{ 2 }O }_{ \left( s \right)  }\rightarrow { 2Ag }_{ \left( s \right)  }+\dfrac { 1 }{ 2 } O_{ 2\left( g \right)  }$$Which of the following statements is true?

Mayuri was performing thermometric titration and she took 100 ml of $$1 M$$ sulphuric acid and started adding $$1 M$$ calcium hydroxide. When she plotted a graph of temperature vs volume of the titrant added, she found that the temperature was initially increasing and then it started decreasing. The maximum of the graph is obtained at 100 ml of calcium hydroxide. What will be the enthalpy change of this reaction?

$$(CH_3)_2CH + Cl_2 \longrightarrow (CH_3)_2CHCl + Cl$$
$$CH_3CH_2CH_2 - H$$                           $$98$$
$$(CH_3)_2CH - H$$                                $$95$$
$$Cl - Cl$$                                               $$58$$
$$H - Cl$$                                                $$103$$
$$CH_3CH_2CH_2 - Cl$$                           $$81$$
$$(CH_3)_2CH -Cl$$                               $$80$$
Given the bond dissociation energies below (in $$kcal/mole$$), estimate the $${ \Delta H }^{ o }$$ for the propagation step:

$$aA + bB \rightleftharpoons cC + dD$$