Gibbs Free Energy (G)

If $∆\mathrm{G}$ for a reaction is negative, the change is:

What are the conditions required for the non-spontaneous endothermic reaction when the change in entropy is positive?

What is the condition for non-spontaneous exothermic reaction?

In which case the reaction is a exothermic spontaneous process?

The efficiency of the fuel cell will be

If $\mathrm{K}<1.0$, what will be the value of $∆\mathrm{G}°$ out of the following ?

Calculate$∆\mathrm{G}$for the reaction at $25°\mathrm{C} \mathrm{CO} \left(\mathrm{g}\right) + 2{\mathrm{H}}_2 \left(\mathrm{g}\right) \to {\mathrm{CH}}_3\mathrm{OH} \left(\mathrm{g}\right) ∆\mathrm{G}° = -24.8 \mathrm{kJ} {\mathrm{mol}}^{-1}$.

If ${\mathrm{P}}_{\mathrm{CO}}=4\mathrm{atm},{\mathrm{P}}_{{\mathrm{H}}_2}=2\mathrm{atm},{\mathrm{P}}_{{\mathrm{CH}}_3\mathrm{OH}}=2\mathrm{atm}$

$\mathrm{Kp}$ for the reaction,${\mathrm{MgCO}}_3 \left(\mathrm{s}\right) \to \mathrm{MgO} \left(\mathrm{s}\right) + {\mathrm{CO}}_2 \left(\mathrm{g}\right) \mathrm{is} 9\mathrm{x}{10}^{-10}$. Calculate $∆\mathrm{G}°$ for the reaction at $25°\mathrm{C}$.

Calculate$\mathrm{Kp}$ for the reaction, ${\mathrm{C}}_2{\mathrm{H}}_4 \left(\mathrm{g}\right) +{\mathrm{H}}_2 \left(\mathrm{g}\right) \to {\mathrm{C}}_2{\mathrm{H}}_6 \left(\mathrm{g}\right), ∆\mathrm{G}° = -100 \mathrm{kJ} {\mathrm{mol}}^{-1} \mathrm{at} 25°\mathrm{C}.$

The relationship between $∆\mathrm{G}°$ of a reaction and its equilibrium constant is

If for a reaction $∆\mathrm{H}$is negative and $∆\mathrm{S}$ is positive then the reaction is

What can be said about the spontaneity of reaction when $∆\mathrm{H}$ is negative and $∆\mathrm{S}$ is positive.

What can be said about the spontaneity of reaction when $∆\mathrm{H}$ is positive and $∆\mathrm{S}$ is negative.

What can be said about the spontaneity of reaction when $∆\mathrm{H}$ and $∆\mathrm{S}$ are both negative.

What can be said about the spontaneity of reaction when $∆\mathrm{H}$ and $∆\mathrm{S}$ are both positive.

Is it possible for a reaction to be non-spontaneous yet exothermic? Explain with example.

It is possible for a reaction to be spontaneous yet endothermic. Comment with example.

Determine whether the following reaction is spontaneous under standard conditions.
$2{\mathrm{H}}_2\mathrm{O} \left(l\right) + {\mathrm{O}}_2 \left(\mathrm{g}\right) \to 2{\mathrm{H}}_2{\mathrm{O}}_2 \left(l\right) ∆\mathrm{H}° =+196 \mathrm{kJ}, ∆\mathrm{S}° = -126 \mathrm{JK}{ }^{–1}$

Does it have a cross-over temperature?

Determine whether the following reaction will be spontaneous or nonspontaneous under standard
conditions.

$\mathrm{Zn} \left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right) \to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right) + \mathrm{Cu} \left(\mathrm{s}\right) ∆H° = -219 \mathrm{kJ}, ∆S° = -21 J K^{-1}.$