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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 76
Capitolo 15, Problema 76

A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(g) ⇌ 2 NO(g) + Br2(g). An equilibrium mixture in a 5.00-L vessel at 100 _x001F_C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br2. (a) Calculate Kc.

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First, convert the masses of NOBr, NO, and Br2 to moles using their respective molar masses. Use the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \).
Next, calculate the concentrations of each species in the equilibrium mixture. Since the volume of the vessel is 5.00 L, use the formula: \( \text{concentration (M)} = \frac{\text{moles}}{\text{volume (L)}} \).
Write the expression for the equilibrium constant \( K_c \) for the reaction: \( K_c = \frac{[\text{NO}]^2[\text{Br}_2]}{[\text{NOBr}]^2} \).
Substitute the concentrations of NO, Br2, and NOBr into the \( K_c \) expression. Ensure that the concentrations are raised to the power of their stoichiometric coefficients.
Finally, solve the expression to find the value of \( K_c \). This will give you the equilibrium constant for the reaction at the given temperature.

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients], where the concentrations are in mol/L. A larger Kc indicates a greater concentration of products at equilibrium, while a smaller Kc suggests that reactants are favored.
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Equilibrium Constant Expressions

Molar Mass and Conversion to Molarity

To calculate Kc, it is essential to convert the mass of each substance into moles using their molar masses. Molarity (M) is then determined by dividing the number of moles by the volume of the solution in liters. This step is crucial because Kc is based on concentrations, and accurate conversion ensures correct equilibrium calculations.
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Molar Mass Concept

Stoichiometry of the Reaction

Understanding the stoichiometry of the reaction is vital for determining the correct coefficients when calculating Kc. In the given reaction, 2 moles of NOBr decompose to produce 2 moles of NO and 1 mole of Br2. The stoichiometric coefficients directly influence the equilibrium expression, as they dictate how the concentrations of each species are related in the Kc calculation.
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Domanda del libro di testo

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (c) According to Le Châtelier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

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Domanda del libro di testo

A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) An equilibrium mixture in a 5.00-L vessel at 100°C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br2. (b) What is the total pressure exerted by the mixture of gases?

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Domanda del libro di testo

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.

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Domanda del libro di testo

A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(g) ⇌ 2 NO(g) + Br2(g) An equilibrium mixture in a 5.00-L vessel at 100°C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br2. (c) What was the mass of the original sample of NOBr?

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