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Chapter 17: Problem 63

What is implied by the word constant in the term equilibrium constant? Give two reaction parameters that can be changed without changing the value of an equilibrium constant.

Short Answer

Expert verified
The term 'constant' implies a fixed value at a given temperature. Reaction parameters like the presence of a catalyst and temperature can be changed without affecting the equilibrium constant.

Step by step solution

01

Understanding the Term 'Constant' in Equilibrium Constant

The term 'constant' in equilibrium constant implies that the value of the equilibrium constant (\(K_{eq}\)) remains unchanged at a given temperature. It is a fixed value that describes the ratio of concentrations of products to reactants when a chemical reaction is at equilibrium.
02

Effect of Temperature

One reaction parameter that can be changed without altering the equilibrium constant is temperature. Temperature changes can affect the rate at which equilibrium is reached, but the value of the equilibrium constant remains the same at a specific temperature.
03

Effect of Catalysts

Another reaction parameter that can be changed without changing the value of the equilibrium constant is the presence of a catalyst. Catalysts speed up the rate at which equilibrium is achieved but do not affect the equilibrium constant value.

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Key Concepts

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

chemical equilibrium
Chemical equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. One important thing to note is that this does not mean the reactants and products are in equal concentrations; it simply means their rates of formation are equal. This balance results in a stable mix as long as the system remains undisturbed. The equilibrium constant (K_{eq}) provides a snapshot of this balance by relating the concentrations of the products to the reactants at equilibrium.
reaction parameters
Reaction parameters are various conditions that can affect how a reaction proceeds and eventually reaches equilibrium.
Some key reaction parameters include:
  • Concentration of Reactants and Products
  • Pressure (especially for gaseous reactions)
  • Volume
  • Temperature
  • Presence of Catalysts
By manipulating these reaction parameters, you can influence the rate of the reaction and how quickly it reaches equilibrium. However, not all parameters will change the equilibrium constant (K_{eq}).
catalysts
Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They achieve this by lowering the activation energy required for the reaction to proceed. While a catalyst can help a reaction reach equilibrium faster, it **does not** change the equilibrium constant (K_{eq}). This means that the final balance of products and reactants remains the same, only achieved more rapidly.
temperature effect
Temperature plays a crucial role in chemical reactions and their equilibria. Changing the temperature of a system can affect both the reaction rate and the equilibrium position. However, the equilibrium constant (K_{eq}) is typically defined for a specific temperature. Once that temperature is set, K_{eq} remains constant. Thus, altering the temperature changes the speed but not the end state of equilibrium, unless the temperature changes significantly alter the kinetic energy and reaction pathways.

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Most popular questions from this chapter

Sodium bicarbonate undergoes thermal decomposition according to the reaction $$ 2 \mathrm{NaHCO}_{3}(s) \Longrightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ How does the equilibrium position shift as a result of each of the following disturbances? (a) 0.20 atm of argon gas is added. (b) \(\mathrm{NaHCO}_{3}(s)\) is added. (c) \(\mathrm{Mg}\left(\mathrm{ClO}_{4}\right)_{2}(s)\) is added as a drying agent to remove \(\mathrm{H}_{2} \mathrm{O}\). (d) Dry ice is added at constant \(T\)

As an EPA scientist studying catalytic converters and urban smog, you want to find \(K_{c}\) for the following reaction: $$ 2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2}(g)+2 \mathrm{O}_{2}(g) \quad K_{\mathrm{c}}=? $$ Use the following data to find the unknown \(K_{\mathrm{c}}\) : $$ \begin{aligned} \frac{1}{2} \mathrm{~N}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \rightleftharpoons \mathrm{NO}(g) & & K_{\mathrm{c}}=4.8 \times 10^{-10} \\ 2 \mathrm{NO}_{2}(g) & \Longrightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) & & K_{\mathrm{c}}=1.1 \times 10^{-5} \end{aligned} $$

For the following reaction, \(K_{c}=115\) at a particular temperature: $$ \mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g) $$ A container initially holds the following concentrations: \(0.050 \mathrm{M}\) \(\mathrm{H}_{2}, 0.050 \mathrm{M} \mathrm{F}_{2},\) and \(0.10 \mathrm{M} \mathrm{HF} .\) When equilibrium is reached, what is the concentration of HF?

Isolation of Group \(8 \mathrm{~B}(10)\) elements, used as industrial catalysts, involves a series of steps. For nickel, the sulfide ore is roasted in air: \(\mathrm{Ni}_{3} \mathrm{~S}_{2}(s)+\mathrm{O}_{2}(g) \rightleftharpoons \mathrm{NiO}(s)+\mathrm{SO}_{2}(g) .\) The metal oxide is reduced by the \(\mathrm{H}_{2}\) in water gas \(\left(\mathrm{CO}+\mathrm{H}_{2}\right)\) to impure \(\mathrm{Ni}: \mathrm{NiO}(s)+\mathrm{H}_{2}(g) \rightleftharpoons \mathrm{Ni}(s)+\mathrm{H}_{2} \mathrm{O}(g) .\) The \(\mathrm{CO}\) in water gas then reacts with the metal in the Mond process to form gaseous nickel carbonyl, \(\mathrm{Ni}(s)+\mathrm{CO}(g) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(g),\) which is sub- sequently decomposed to the metal. (a) Balance each of the three steps, and obtain an overall balanced equation for the conversion of \(\mathrm{Ni}_{3} \mathrm{~S}_{2}\) to \(\mathrm{Ni}(\mathrm{CO})_{4}\). (b) Show that the overall \(Q_{\mathrm{c}}\) is the product of the \(Q_{c}\) 's for the individual reactions.

A change in reaction conditions increases the rate of a certain forward reaction more than that of the reverse reaction. What is the effect on the equilibrium constant and on the concentrations of reactants and products at equilibrium?
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