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Chapter 14: Problem 73

Consider the equilibrium $$ \mathrm{FeO}(s)+\mathrm{CO}(g) \rightleftharpoons \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) $$ When carbon dioxide is removed from the equilibrium mixture (say, by passing the gases through water to absorb \(\mathrm{CO}_{2}\) ), what is the direction of net reaction as the new equilibrium is achieved?

Short Answer

Expert verified
The net reaction shifts to the right to produce more CO鈧�.

Step by step solution

01

Understand Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. When CO鈧� is removed, the system will shift to produce more CO鈧� to replace the loss.
02

Analyze the Reaction

The given reaction is: \[\mathrm{FeO}(s)+\mathrm{CO}(g) \rightleftharpoons \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)\]In this reaction, removing CO鈧� will cause the equilibrium to shift to the right to produce more CO鈧�.
03

Predict the Direction of Shift

Since CO鈧� is a product, removing it will decrease its concentration in the system. According to Le Chatelier's principle, the equilibrium will shift to the right towards the products to increase the concentration of CO鈧�.
04

Confirm the Net Reaction Shift

When CO鈧� is removed, the system compensates for the change by moving the equilibrium towards the right. This increases the formation of products (\(\mathrm{Fe}(s)\) and \(\mathrm{CO}_{2}(g)\)) and consumes more reactants (\(\mathrm{FeO}(s)\) and \(\mathrm{CO}(g)\)).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Equilibrium
Chemical equilibrium occurs in a closed system where the rates of the forward and reverse reactions are equal. While reactions continue to occur, there is no net change in the concentration of reactants and products.

At equilibrium, the system is stable, but dynamic. This means molecules are constantly moving and reacting. However, the overall composition remains unchanged if the conditions remain constant.

Understanding chemical equilibrium is crucial for analyzing how systems respond to changes, such as alterations in concentrations or pressure, using concepts such as Le Chatelier's Principle.
Reaction Direction
The direction of a reaction can shift depending on various factors. Le Chatelier's Principle helps us predict this shift. It states that when a system at equilibrium is subjected to a change鈥攍ike concentration, pressure, or temperature鈥攖he system will adjust to offset that change.

In the given reaction:
  • Addition of \( ext{CO}_2\) shifts the reaction towards the reactants (left).
  • Removal of \( ext{CO}_2\) shifts the reaction towards the products (right).
Understanding the reaction direction helps to determine how reaction conditions must be manipulated to obtain a desired level of product.
Equilibrium Shift
Equilibrium shift happens when a system at equilibrium responds to a change in conditions by adjusting concentrations of reactants and products.

In the context of the reaction \( ext{FeO}(s) + ext{CO}(g) \rightleftharpoons ext{Fe}(s) + ext{CO}_{2}(g)\), removing \( ext{CO}_2\) results in an equilibrium shift to the right. The system reacts by "producing" more \( ext{CO}_2\) to counteract its removal.
  • This shift increases the amount of \( ext{Fe}(s)\) and \( ext{CO}_2\).
  • Conversely, \( ext{FeO}(s)\) and \( ext{CO}(g)\) are consumed more.
Equilibrium shifts are predictable, allowing chemists to control and optimize reaction conditions.
Dynamic Equilibrium
Dynamic equilibrium is a state where the forward and reverse reactions occur at the same rate, resulting in no net change in reactant and product concentrations.

Despite the equilibrium, substances are constantly transforming. For instance, \( ext{FeO}(s)\) and \( ext{CO}(g)\) continuously react to form \( ext{Fe}(s)\) and \( ext{CO}_2(g)\), while the reverse reaction occurs simultaneously.

Changes, like removing \( ext{CO}_2\), disturb this balance. However, the dynamic nature allows the system to respond by adjusting its concentrations, eventually establishing a new equilibrium. This highlights the resilience and adaptability of chemical equilibria.

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Most popular questions from this chapter

For each of the following equations, give the expression for the equilibrium constant \(K_{c}\) $$ \begin{array}{l} \text { a } \mathrm{NH}_{4} \mathrm{Cl}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \\ \text { b } \mathrm{C}(s)+2 \mathrm{~N}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+2 \mathrm{~N}_{2}(g) \\ \text { c } \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{NaHCO}_{3}(s) \\\ \text { d } \mathrm{Fe}^{3+}(a q)+3 \mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{Fe}(\mathrm{OH})_{3}(s) \end{array} $$

The equilibrium-constant expression for a reaction is $$ K_{c}=\frac{\left[\mathrm{NO}_{2}\right]^{4}\left[\mathrm{O}_{2}\right]}{\left[\mathrm{N}_{2} \mathrm{O}_{5}\right]^{2}} $$ What is the equilibrium-constant expression when the equation for this reaction is halved and then reversed?

An equilibrium mixture of \(\mathrm{SO}_{3}, \mathrm{SO}_{2},\) and \(\mathrm{O}_{2}\) at $$ 727^{\circ} \mathrm{C} \text { is } 0.0160 \mathrm{M} \mathrm{SO}_{3}, 0.0056 \mathrm{M} \mathrm{SO}_{2} \text { , and } 0.0021 \mathrm{M} \mathrm{O}_{2} $$ What is the value of \(K_{c}\) for the following reaction? $$ \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g) $$

What would you expect to be the effect of an increase of pressure on each of the following reactions? Would the pressure change cause the reaction to go to the right or left? $$ \begin{array}{l} \text { a } \mathrm{CH}_{4}(g)+2 \mathrm{~S}_{2}(g) \rightleftharpoons \mathrm{CS}_{2}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g) \\ \text { b } \mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{HBr}(g) \\ \text { c } \mathrm{CO}_{2}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{CO}(g) \end{array} $$

How is it possible for a catalyst to give products from a reaction mixture that are different from those obtained when no catalyst or a different catalyst is used? Give an example.
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