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Chapter 16: Q16.4-64E (page 913)

Without doing a numerical calculation, determine which of the following will reduce the free energy change for the reaction, that is, make it less positive or more negative, when the temperature is increased. Explain.

(a) \({{\bf{N}}_{\bf{2}}}{\bf{(g) + 3}}{{\bf{H}}_{\bf{2}}}{\bf{(g)}} \to {\bf{2N}}{{\bf{H}}_{\bf{3}}}{\bf{(g)}}\)

(b) \({\bf{HCl(g) + N}}{{\bf{H}}_{\bf{3}}}{\bf{(g)}} \to {\bf{N}}{{\bf{H}}_{\bf{4}}}{\bf{Cl(s)}}\)

(c) \({\left( {{\bf{N}}{{\bf{H}}_{\bf{4}}}} \right)_{\bf{2}}}{\bf{C}}{{\bf{r}}_{\bf{2}}}{{\bf{O}}_{\bf{7}}}{\bf{(s)}} \to {\bf{C}}{{\bf{r}}_{\bf{2}}}{{\bf{O}}_{\bf{3}}}{\bf{(s) + 4}}{{\bf{H}}_{\bf{2}}}{\bf{O(g) + }}{{\bf{N}}_{\bf{2}}}{\bf{(g)}}\)

(d) \({\bf{2Fe(s) + 3}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}} \to {\bf{F}}{{\bf{e}}_{\bf{2}}}{{\bf{O}}_{\bf{3}}}{\bf{(s)}}\)

Short Answer

Expert verified

Option B is correct answer \({\rm{HCl}}(g) + {\rm{N}}{{\rm{H}}_3}(g) \to {\rm{N}}{{\rm{H}}_4}{\rm{Cl}}(s)\)

Step by step solution

01

Define exothermic reaction and endothermic reaction

The spontaneity of a reaction depends on the releasing or absorption of energy. If the amount of energy releases during the reaction, then the reaction is exothermic reactionwhile the amount of energy absorbed during the reaction then the reaction isendothermic reaction. The value of enthalpy is positive for endothermic reaction while value of enthalpy is negative for exothermic reaction.

02

Reason for correct option.

The given reaction for the production of ammonium chloride is endothermic reaction with value \(64.81\;{\rm{kJ}}\) /mol. The reaction continuously absorbs the heat for the yielding of product. On increasing the temperature, the reaction goes in forward direction toward the product. Thus, the reaction become spontaneous and makes the Gibbs value more negative.

Hence, option (b) is correct.

03

Reason for incorrect option.

The given reaction for the production of ammonia is exothermic reaction with value \( - 46.28\;{\rm{kJ}}/{\rm{mol}}\). The reaction continuously releases the heat for the yielding of product. On increasing the temperature, the reaction goes in reverse direction toward the reactant. Thus, the reaction become non spontaneous and makes the Gibbs value more positive.

The given reaction for the production of alumina chromium is exothermic reaction with value \( - 272.8\;{\rm{kJ}}/{\rm{mol}}\). The reaction continuously releases the heat for the yielding of product. On increasing the temperature, the reaction goes in reverse direction toward the reactant. Thus, the reaction become non spontaneous and makes the Gibbs value more positive.

The given reaction for the production of Iron oxide is exothermic reaction with value \( - 850.72\;{\rm{kJ}}/{\rm{mol}}\). The reaction continuously releases the heat for the yielding of product. On increasing the temperature, the reaction goes in reverse direction toward the reactant. Thus, the reaction become non spontaneous and makes the Gibbs value more positive.

Hence, option (a), (c), (d) are incorrect.

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Most popular questions from this chapter

Predict the sign of the enthalpy change for the following processes. Give a reason for your prediction.

(a) \({\bf{NaN}}{{\bf{O}}_{\bf{3}}}{\bf{(s)}} \to {\bf{N}}{{\bf{a}}^{\bf{ + }}}{\bf{(aq) + N}}{{\bf{O}}_{\bf{3}}}^{\bf{ - }}{\bf{(aq)}}\)

(b) the freezing of liquid water

(c) \({\bf{C}}{{\bf{O}}_{\bf{2}}}{\bf{(s)}} \to {\bf{C}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

(d) \({\bf{CaCO(s)}} \to {\bf{CaO(s) + C}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

Consider the decomposition of red mercury(II) oxide under standard state conditions.

\({\bf{2HgO(s, red )}} \to {\bf{2Hg(l) + }}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

(a) Is the decomposition spontaneous under standard state conditions?

(b) Above what temperature does the reaction become spontaneous?

Is the formation of ozone \(\left( {{{\bf{O}}_{\bf{3}}}{\bf{(g)}}} \right)\) from oxygen \(\left( {{{\bf{O}}_{\bf{2}}}{\bf{(g)}}} \right)\) spontaneous at room temperature under standard state conditions?

Many plastic materials are organic polymers that contain carbon and hydrogen. The oxidation of these plastics in air to form carbon dioxide and water is a spontaneous process; however, plastic materials tend to persist in the environment. Explain.

One of the important reactions in the biochemical pathway glycolysis is the reaction of glucose-6-phosphate (G6P) to form fructose-6-phosphate (F6P):

\({\text{G}}6{\text{P}} \rightleftharpoons {\text{F}}6{\text{P}}\;\;\;\Delta G_{298}^\circ = 1.7\;{\text{kJ}}\)

(a) Is the reaction spontaneous or nonspontaneous under standard thermodynamic conditions?

(b) Standard thermodynamic conditions imply the concentrations of G6P and F6P to be \(1M\), however, in a typical cell, they are not even close to these values. Calculate \(\Delta G\)when the concentrations of G6P and F6P are \(120\mu M\) and \(28\mu M\)respectively, and discuss the spontaneity of the forward reaction under these conditions. Assume the temperature is 37掳C
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