/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 6 Ethene \(\left(\mathrm{C}_{2} \m... [FREE SOLUTION] | 91影视

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Chapter 15: Problem 6

Ethene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\) reacts with halogens \(\left(\mathrm{X}_{2}\right)\) by the following reaction: $$ \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{X}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{X}_{2}(g) $$ The following figures represent the concentrations at equilibrium at the same temperature when \(\mathrm{X}_{2}\) is \(\mathrm{Cl}_{2}\) (green), \(\mathrm{Br}_{2}\) (brown), and \(\mathrm{I}_{2}\) (purple). List the equilibria from smallest to largest equilibrium constant. [Section 15.3]

Short Answer

Expert verified
The equilibria can be ordered from smallest to largest equilibrium constant as follows: \(K_\text{I鈧倉 \lt K_\text{Br鈧倉 \lt K_\text{Cl鈧倉\) based on the given information about equilibrium concentrations for each reaction with halogens.

Step by step solution

01

Understanding the equilibrium constant

The equilibrium constant (K) for a reaction is the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium. In this case, our reaction is: $$ \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{X}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{X}_{2}(g) $$ So, the equilibrium constant (K) can be expressed as: $$ K = \frac{[\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{X}_{2}]_{eq}}{[\mathrm{C}_{2} \mathrm{H}_{4}]_{eq}\cdot[\mathrm{X}_{2}]_{eq}} $$ Notice that in this reaction, all species are in gaseous form.
02

Calculate the equilibrium constant for each halogen

We are given the equilibrium concentrations of reactants and products for each halogen. To calculate the equilibrium constant for each halogen, we can simply plug the concentrations into the K expression and calculate K.
03

Compare the equilibrium constants

Once we have the equilibrium constants for each halogen, we can order them from smallest to largest as requested in the exercise. For the given information, we can see that the equilibrium concentration for C鈧侶鈧刋鈧� is highest when reacting with Cl鈧�, slightly lower when reacting with Br鈧�, and lowest when reacting with I鈧�. The equilibrium concentration of the reactants C鈧侶鈧� and X鈧� increases in the order Cl鈧�, Br鈧�, and I鈧�. So, we can determine the order of the equilibrium constants without actually calculating the K values. Ordering the equilibrium constants from smallest to largest based on the given information: $$ K_\text{I鈧倉 \lt K_\text{Br鈧倉 \lt K_\text{Cl鈧倉 $$

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Most popular questions from this chapter

Which of the following statements are true and which are false? (a) For the reaction \(2 \mathrm{~A}(g)+\mathrm{B}(g) \rightleftharpoons \mathrm{A}_{2} \mathrm{~B}(g) K_{c}\) and \(K_{p}\) are numerically the same. (b) It is possible to distinguish \(K_{c}\) from \(K_{p}\) by comparing the units used to express the equilibrium constant. (c) For the equilibrium in (a), the value of \(K_{c}\) increases with increasing pressure.

At \(800 \mathrm{~K}\), the equilibrium constant for \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(\mathrm{g})\) is \(K_{c}=3.1 \times 10^{-5}\). If an equilibrium mixture in a 10.0-L vessel contains \(2.67 \times 10^{-2} \mathrm{~g}\) of \(\mathrm{I}(\mathrm{g})\), how many grams of \(\mathrm{I}_{2}\) are in the mixture?

The protein hemoglobin (Hb) transports \(\mathrm{O}_{2}\) in mammalian blood. Each \(\mathrm{Hb}\) can bind \(4 \mathrm{O}_{2}\) molecules. The equilibrium constant for the \(\mathrm{O}_{2}\) binding reaction is higher in fetal hemoglobin than in adult hemoglobin. In discussing protein oxygen-binding capacity, biochemists use a measure called the P50 value, defined as the partial pressure of oxygen at which \(50 \%\) of the protein is saturated. Fetal hemoglobin has a P50 value of 19 torr, and adult hemoglobin has a P50 value of \(26.8\) torr. Use these data to estimate how much larger \(K_{c}\) is for the aqueous reaction \(4 \mathrm{O}_{2}(g)+\mathrm{Hb}(a q) \longrightarrow\) \(\left[\mathrm{Hb}\left(\mathrm{O}_{2}\right)_{4}(a q)\right] .\)

For the equilibrium $$ \mathrm{Br}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{BrCl}(g) $$ at \(400 \mathrm{~K}, K_{c}=7.0\). If \(0.25 \mathrm{~mol}\) of \(\mathrm{Br}_{2}\) and \(0.55 \mathrm{~mol}\) of \(\mathrm{Cl}_{2}\) are introduced into a \(3.0-\mathrm{L}\) container at \(400 \mathrm{~K}\), what will be the equilibrium concentrations of \(\mathrm{Br}_{2}, \mathrm{Cl}_{2}\), and \(\mathrm{BrCl}\) ?

Methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: \(\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\). An equilibrium mixture in a \(2.00\) - L vessel is found to contain \(0.0406 \mathrm{~mol}\) \(\mathrm{CH}_{3} \mathrm{OH}, 0.170 \mathrm{~mol} \mathrm{CO}\), and \(0.302 \mathrm{~mol} \mathrm{H}\) at \(500 \mathrm{~K}\). Calculate \(K_{c}\) at this temperature.
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