Skip to main content
Ch.19 - Chemical Thermodynamics
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.19 - Chemical ThermodynamicsProblema 96c
Capitolo 19, Problema 96c

(c) In each case, indicate whether K should increase or decrease with increasing temperature. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)

Guida verificata passo dopo passo
1
Identify the type of reaction for each case: exothermic or endothermic. This can often be inferred from the reaction equation or given data.
Apply Le Chatelier's Principle: For an exothermic reaction, increasing temperature shifts the equilibrium to the left, decreasing K. For an endothermic reaction, increasing temperature shifts the equilibrium to the right, increasing K.
For reaction (i) 2 Mg(s) + O2(g) ⇌ 2 MgO(s), determine if the formation of MgO is exothermic or endothermic. Typically, the formation of metal oxides is exothermic.
For reaction (ii) 2 KI(s) ⇌ 2 K(g) + I2(g), consider the phase change from solid to gas, which usually requires energy input, indicating an endothermic process.
For reactions (iii) Na2(g) ⇌ 2 Na(g) and (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g), analyze the stoichiometry and phase changes to determine the enthalpy change, and apply Le Chatelier's Principle accordingly.

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:
3m

Concetti chiave

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

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how the equilibrium constant (K) will respond to changes in temperature, pressure, or concentration. For example, if a reaction is exothermic, increasing the temperature will shift the equilibrium to favor the reactants, thus decreasing K.
Video consigliato:
Percorso guidato
07:32
Le Chatelier's Principle

Endothermic and Exothermic Reactions

Reactions can be classified as endothermic or exothermic based on their heat exchange with the surroundings. Endothermic reactions absorb heat, while exothermic reactions release heat. The temperature dependence of the equilibrium constant K is influenced by the nature of the reaction; for endothermic reactions, increasing temperature increases K, while for exothermic reactions, it decreases K.
Video consigliato:
Percorso guidato
02:30
Endothermic & Exothermic Reactions

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It provides insight into the extent of a reaction and how it shifts in response to changes in conditions. Understanding how K varies with temperature is crucial for predicting the direction of a reaction's shift when temperature changes.
Video consigliato:
Percorso guidato
01:14
Equilibrium Constant K
Pratica correlata
Domanda del libro di testo

The potassium-ion concentration in blood plasma is about 5.0⨉10-3 M, whereas the concentration in muscle-cell fluid is much greater (0.15 M ). The plasma and intracellular fluid are separated by the cell membrane, which we assume is permeable only to K+. (a) What is ΔG for the transfer of 1 mol of K+ from blood plasma to the cellular fluid at body temperature 37 °C? (b) What is the minimum amount of work that must be used to transfer this K+?

1097
views
1
rank
Domanda del libro di testo

Using the data in Appendix C and given the pressures listed, calculate Kp and ΔG for each of the following reactions:

(a) N2(g) + 3 H2(g) → 2 NH3(g) PN2 = 2.6 atm, PH2 = 5.9 atm, PNH3 = 1.2 atm

(b) 2 N2H4(g) + 2 NO2(g) → 3 N2(g) + 4 H2O(g) PN2H4 = PNO2 = 5.0 × 10-2 atm, PN2 = 0.5 atm, PH2O = 0.3 atm

(c) N2H4(g) → N2(g) + 2 H2(g) PN2H4 = 0.5 atm, PN2 = 1.5 atm, PH2 = 2.5 atm

807
views
Domanda del libro di testo

At what temperatures is the following reaction, the reduction of magnetite by graphite to elemental iron, spontaneous? Fe3O4(s) + 2 C(s, graphite) → 2 CO2(g) + 3 Fe(s)

795
views
1
comments
Domanda del libro di testo

(a) For each of the following reactions, predict the sign of ΔH° and ΔS° without doing any calculations. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)

860
views
Domanda del libro di testo

The conversion of natural gas, which is mostly methane, into products that contain two or more carbon atoms, such as ethane (C2H6), is a very important industrial chemical process. In principle, methane can be converted into ethane and hydrogen: 2 CH4(g) → C2H6(g) + H2(g) In practice, this reaction is carried out in the presence of oxygen: 2 CH4(g) + 12 O2(g) → C2H6(g) + H2O(g) (b) Is the difference in ΔG° for the two reactions due primarily to the enthalpy term (ΔH) or the entropy term (-TΔS)?

407
views
Domanda del libro di testo

(b) Based on your general chemical knowledge, predict which of these reactions will have K>1. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)

369
views