Thermodynamics ...

A large positive value of $$\Delta { G }$$ corresponds to which of these?

Under which circumstances would the free energy change for a reaction be relatively temperature independent?

$$2Zn+{ O }_{ 2 }\longrightarrow 2ZnO;\Delta { G }^{ o }=-616J..(i)\quad $$
$$2Zn+2S\longrightarrow 2ZnS;\Delta { G }^{ o }=-293J...(ii)$$
$$2S+2{ O }_{ 2 }\longrightarrow 2S{ O }_{ 2 }(g);\Delta { G }^{ o }=-408J..(iii)$$
$$\Delta { G }^{ o }$$ for the following reaction:
$$2ZnS+3{ O }_{ 2 }\longrightarrow 2ZnO+2{ SO }_{ 2 }$$ would be:

The value of $$\log _{ 10 }{ K } $$ for a reaction
 $$A\rightleftharpoons B$$ is____________.
Given $${ \Delta  }_{ r }{ H }_{ 298K }^{ o }=-54.07kJ{ mol }^{ -1 },{ \Delta  }_{ r }{ S }_{ 298K }^{ o }=10J{ K }^{ -1 }{ mol }^{ -1 },R=8.314J{ K }^{ -1 }{ mol }^{ -1 }$$

Given that:
$$2C(s)+2{ O }_{ 2 }(g)\longrightarrow 2C{ O }_{ 2 }(g);\Delta H=-787kJ...(i)$$
$${ H }_{ 2 }(g)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow { H }_{ 2 }O(l);\Delta H=-286kJ...(ii)$$
$${ C }_{ 2 }{ H }_{ 2 }(g)+\cfrac { 5 }{ 2 } { O }_{ 2 }(g)\longrightarrow 2C{ O }_{ 2 }(g)+3{ H }_{ 2 }O(l)....(iii)$$
$$\Delta H=-1301kJ$$
Heat formation of acetylene is:

The enthalpy changes for two reactions are given by the equations:
$$2Cr(s)+1\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow { Cr }_{ 2 }{ O }_{ 3 }(s);\Delta H=-1130kJ$$
$$C(s)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow CO(g);\Delta H=-110kJ$$
What is the enthalpy change, in $$kJ$$, for the reaction?
$$3C(s)+{ Cr }_{ 2 }{ O }_{ 3 }(s)\longrightarrow 2Cr(s)+3CO(g)$$

The enthalpy change for two reactions are given by the equations:
$$2Cr(s)+\cfrac { 3 }{ 2 } { O }_{ 2 }(g)\longrightarrow { Cr }_{ 2 }{ O }_{ 3 }(s);\Delta H=-1130kJ$$
$$C(s)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow CO(g);\Delta H=-110kJ$$
What is the enthalpy change in $$kJ$$ for the following reaction?
$$3C(s)+{ Cr }_{ 2 }{ O }_{ 3 }(s)\longrightarrow 2Cr(s)+3CO(g)$$

Given that:
$$2Fe(s)+\cfrac { 3 }{ 2 } { O }_{ 2 }(g)\longrightarrow { Fe }_{ 2 }{ O }_{ 3 }(s);\Delta H=-193.4kJ...(i)$$
$$Mg(s)+\cfrac { 1 }{ 2 } { O }_{ 2 }(g)\longrightarrow MgO(s);\Delta H=-140.2kJ....(ii)$$
What is $$\Delta H$$ of the reaction?
$$3Mg+{ Fe }_{ 2 }{ O }_{ 3 }\longrightarrow 3MgO+2Fe$$

 A 100.0g ice cube at 0.0°C is placed in 650g of water at 25°C. What is the final temperature of the mixture?

For spontaneous process: