Skip to main content
Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.15 - Chemical EquilibriumProblema 39
Capitolo 15, Problema 39

Consider the reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g) Kp = 28.4 at 298K In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture?

Guida verificata passo dopo passo
1
Step 1: Understand the problem. We are given the equilibrium constant (Kp) for the reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g) and the partial pressures of NO and Br2. We need to find the partial pressure of NOBr.
Step 2: Write down the expression for the equilibrium constant (Kp) for the given reaction. Kp = [NOBr]^2 / ([NO]^2 * [Br2])
Step 3: Convert the given pressures from torr to atmospheres because the equilibrium constant is usually given in terms of atmospheres. 1 atm = 760 torr. So, [NO] = 108 torr / 760 torr/atm and [Br2] = 126 torr / 760 torr/atm.
Step 4: Substitute the known values into the equilibrium expression and solve for [NOBr]. Remember that [NOBr] = sqrt(Kp * [NO]^2 * [Br2]).
Step 5: The result will be the partial pressure of NOBr in atmospheres. If needed, convert it back to torr by multiplying by 760 torr/atm.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2m

Concetti chiave

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

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g), Kp is calculated using the formula Kp = (P_NOBr^2) / (P_NO^2 * P_Br2), where P represents the partial pressures of the gases involved.
Video consigliato:
Percorso guidato
03:20
Equilibrium Constant Expressions

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. It can be determined using Dalton's Law, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual components. In this context, the partial pressures of NO and Br2 are given, and the partial pressure of NOBr needs to be calculated using the equilibrium constant.
Video consigliato:
Percorso guidato
00:48
Partial Pressure Calculation

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In this reaction, if the concentrations of NO or Br2 were to change, the system would shift to either the left or right to re-establish equilibrium, which is relevant when considering how the partial pressures relate to Kp.
Video consigliato:
Percorso guidato
07:32
Le Chatelier's Principle
Pratica correlata
Domanda del libro di testo

Consider the reaction: N2(g) + 3 H2(g) ⇌ 2 NH3(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.

T (K) [N2] [H2] [NH3] Kc

500 0.115 0.105 0.439 _

575 0.110 _ 0.128 9.6

775 0.120 0.140 _ 0.0584

764
views
Domanda del libro di testo

Consider the following reaction: H2(g) + I2(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilibrium concentrations in M.

T (°C) [H2] [I2] [HI] Kc

25 0.0355 0.0388 0.922 _

340 _ 0.0455 0.387 9.6

445 0.0485 0.0468 _ 50.2

1347
views
Domanda del libro di testo

Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91⨉103 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2in this mixture?

1673
views