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Chapter 14: Problem 4

Write the equilibrium constant expression for the reaction \(\mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftarrows \mathrm{CS}_{2}(g)+4 \mathrm{H}_{2}(g)\)

Short Answer

Expert verified
The short answer for the equilibrium constant expression (Kc) for the given reaction \(CH_4(g) + 2 H_2S(g) \rightleftarrows CS_2(g) + 4 H_2(g)\) is: \(K_c = \frac{[CS_2][H_2]^4}{[CH_4][H_2S]^2}\)

Step by step solution

01

Identify the reactants and products

In this given chemical equation, the reactants are methane (CH4) and hydrogen sulfide (H2S). The products are carbon disulfide (CS2) and hydrogen gas (H2).
02

Write the equilibrium expression for each species

For each reactant and product, we will write the equilibrium concentrations using square brackets to represent the concentration of the species at equilibrium. - For CH4: [CH4] - For H2S: [H2S] - For CS2: [CS2] - For H2: [H2]
03

Write the equilibrium constant expression (Kc)

The equilibrium constant expression (Kc) for a reaction is the ratio of the product concentrations raised to their respective stoichiometric coefficients to the reactant concentrations raised to their respective stoichiometric coefficients at equilibrium. In our reaction, \(CH_4(g) + 2 H_2S(g) \rightleftarrows CS_2(g) + 4 H_2(g)\), the stoichiometric coefficients are 1 for CH4, 2 for H2S, 1 for CS2, and 4 for H2. The equilibrium constant expression (Kc) for this reaction will be: \(K_c = \frac{[CS_2]^1[H_2]^4}{[CH_4]^1[H_2S]^2} = \frac{[CS_2][H_2]^4}{[CH_4][H_2S]^2}\) This is the equilibrium constant expression for the given reaction.

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Most popular questions from this chapter

How would the value of the equilibrium constant for a one-step reaction calculated as \(k_{\mathrm{f}} / k_{\mathrm{r}}\) compare with the value calculated from the concentrations of all substances present at equilibrium?

When the reaction \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftarrows 2 \mathrm{NO}(g)\) is run at \(2000^{\circ} \mathrm{C}\), appreciable amounts of reactants and product are present at equilibrium. (a) A sealed 2.00-L container at \(2000{ }^{\circ} \mathrm{C}\) is filled with \(1.00\) mole of \(\mathrm{NO}(g)\) and nothing else. At that moment, which reaction is faster, forward or reverse? Justify your answer. (b) At equilibrium, the concentration of \(\mathrm{NO}(g)\) is \(0.0683 \mathrm{M}\) and the concentration of \(\mathrm{N}_{2}(g)\) is \(0.2159 \mathrm{M}\). What is the value of \(K_{\mathrm{eq}}\) at \(2000^{\circ} \mathrm{C} ?\)

Sparingly soluble calcium phosphate dissolves in water to yield an equilibrium calcium ion concentration of \(7.8 \times 10^{-6} \mathrm{M}\). (a) Write the balanced equilibrium equation for calcium phosphate dissolving in water. (b) Write the \(K_{\text {sp }}\) expression for calcium phosphate. (c) What is the equilibrium concentration of phosphate ion? (d) Calculate the value of \(K_{s p}\) for calcium phosphate (show your calculation).

Sparingly soluble \(\mathrm{PbCl}_{2}\) dissolves in water to yield an equilibrium \(\mathrm{Pb}^{2+}(a q)\) concentration of \(0.039 \mathrm{M}\). (a) Write the balanced equilibrium equation for \(\mathrm{PbCl}_{2}(\) s) dissolving in water. (b) Write the \(K_{\text {sp }}\) expression for \(\mathrm{PbCl}_{2}\). (c) What is the equilibrium concentration of chloride ion? (d) Calculate the value of \(K_{\mathrm{sp}}\) for \(\mathrm{PbCl}_{2}\) (show your calculation).

Consider the two curves, one showing supply of tapes, the other showing demand for tapes. At what price per quantity is equilibrium established?
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