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Chapter 12: Problem 21

Write the equilibrium expression \((K)\) for each of the following gas-phase reactions. a. \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)\). b. \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)\). c. \(\operatorname{SiH}_{4}(g)+2 \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SiCl}_{4}(g)+2 \mathrm{H}_{2}(g)\). d. \(2 \mathrm{PBr}_{3}(g)+3 \mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{PCl}_{3}(g)+3 \mathrm{Br}_{2}(g)\).

Short Answer

Expert verified
The equilibrium expressions for the given gas-phase reactions are as follows: a. \(K = \frac{[NO]^2}{[N2] \times [O2]}\) b. \(K = \frac{[NO2]^2}{[N2O4]}\) c. \(K = \frac{[SiCl4] \times [H2]^2}{[SiH4] \times [Cl2]^2}\) d. \(K = \frac{[PCl3]^2 \times [Br2]^3}{[PBr3]^2 \times [Cl2]^3}\)

Step by step solution

01

Identify the reactants and products

In this reaction, the reactants are Nitrogen gas (N2) and Oxygen gas (O2), while the product is Nitrogen Monoxide gas (NO).
02

Write the equilibrium expression

Now, we will use the formula for the equilibrium expression to write the expression for this reaction: \(K = \frac{[NO]^2}{[N2] \times [O2]}\) #a. Reaction 2: N2O4(g) ⇌ 2 NO2(g)#
03

Identify the reactants and products

In this reaction, the reactant is Dinitrogen Tetroxide (N2O4) and the product is Nitrogen Dioxide gas (NO2).
04

Write the equilibrium expression

Now, we will use the formula for the equilibrium expression to write the expression for this reaction: \(K = \frac{[NO2]^2}{[N2O4]}\) #c. Reaction 3: SiH4(g) + 2 Cl2(g) ⇌ SiCl4(g) + 2 H2(g)#
05

Identify the reactants and products

In this reaction, the reactants are Silicon Tetrahydride (SiH4) and Chlorine gas (Cl2), while the products are Silicon Tetrachloride (SiCl4) and Hydrogen gas (H2).
06

Write the equilibrium expression

Now, we will use the formula for the equilibrium expression to write the expression for this reaction: \(K = \frac{[SiCl4] \times [H2]^2}{[SiH4] \times [Cl2]^2}\) #d. Reaction 4: 2 PBr3(g) + 3 Cl2(g) ⇌ 2 PCl3(g) + 3 Br2(g)#
07

Identify the reactants and products

In this reaction, the reactants are Phosphorus Tribromide (PBr3) and Chlorine gas (Cl2), while the products are Phosphorus Trichloride (PCl3) and Bromine gas (Br2).
08

Write the equilibrium expression

Now, we will use the formula for the equilibrium expression to write the expression for this reaction: \(K = \frac{[PCl3]^2 \times [Br2]^3}{[PBr3]^2 \times [Cl2]^3}\)

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Most popular questions from this chapter

Peptide decomposition is one of the key processes of digestion, where a peptide bond is broken into an acid group and an amine group. We can describe this reaction as follows: \(\text { Peptide }(a q)+\mathrm{H}_{2} \mathrm{O}(t) \rightleftharpoons \text { acid group }(a q)+\text { amine group }(a q)\)

Consider the following reaction at a certain temperature:$$4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)$$.An equilibrium mixture contains 1.0 mole of \(\mathrm{Fe}, 1.0 \times 10^{-3}\) mole of \(\mathrm{O}_{2},\) and 2.0 moles of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) all in a \(2.0-\mathrm{L}\) container. Calculate the value of \(K\) for this reaction.

Suppose the reaction system $$\mathrm{UO}_{2}(s)+4 \mathrm{HF}(g) \rightleftharpoons \mathrm{UF}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$,has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. Additional UO \(_{2}(s)\) is added to the system. b. The reaction is performed in a glass reaction vessel; \(\mathrm{HF}(g)\) attacks and reacts with glass. c. Water vapor is removed.

Lexan is a plastic used to make compact discs, eyeglass lenses, and bulletproof glass. One of the compounds used to make Lexan is phosgene \(\left(\mathrm{COCl}_{2}\right),\) an extremely poisonous gas. Phosgene decomposes by the reaction,$$\operatorname{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)$$,for which \(K_{\mathrm{p}}=6.8 \times 10^{-9}\) at \(100^{\circ} \mathrm{C}\). If pure phosgene at an initial pressure of 1.0 atm decomposes, calculate the equilibrium pressures of all species.

For the reaction \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g), K_{\mathrm{p}}=0.25\) at a certain temperature. If 0.040 atm of \(\mathrm{N}_{2} \mathrm{O}_{4}\) is reacted initially, calculate the equilibrium partial pressures of \(\mathrm{NO}_{2}(g)\) and \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\).
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