2 questions, need help! When the oxide of generic metal M is heated at 25.0 °C,...
When the oxide of generic metal M is heated at 25.0 ∘C , a negligible amount of M is produced. MO2(s)↽−−⇀M(s)+O2(g) Δ?∘ = 291.4kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s) . chemical equation: What is the thermodynamic equilbrium constant for the coupled reaction? ?=
Need help finding K When the oxide of generic metal M is heated at 25.0 degree C, only a negligible amount of M is produced. MO_2(s) rightleftharpoons M(s) + O_2(g) Delta CO_2=291.4 kj/mol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s). What is the thermodynamic equilbrium constant for...
When the oxide of generic metal M is heated at 25.0 ∘C , a negligible amount of M is produced. MO2(s)↽−−⇀M(s)+O2(g) Δ?∘=287.8kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s) . chemical equation: What is the thermodynamic equilbrium constant for the coupled reaction? ?=
When the oxide of generic metal M is heated at 25.0*C, a negligible amount of M is produced. MO,5) = M(s) +0,6) AG* = 2894 When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(8). chemical equation: What is the thermodynamic equilbrium constant for the coupled reaction?
When the oxide of generic metal M is heated at 25.0 °C, only a negligible amount of M is produced.O2M(s) ----> M(s) +O2(g) delta G= 288.9 Kj/molWhen this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(s).I got an answer of :O2M(s)+ C(s) ----> M(s) + CO2(g)This is correct. I need...
I ACCIDENTALLY ASKED THE SAME QUESTION TWICE. PLEASE DO NOT ANSWER A reaction A(aq) +B(aq)C(aq) has a standard free-energy change of-3.38 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? [A] м [B М [C М How would your answers change if the reaction had a standard free-energy change of +3.38 kJ/mol? There would be no...
A reaction A ( aq ) + B ( aq ) − ⇀ ↽ − C ( aq ) has a standard free‑energy change of − 5.46 kJ / mol at 25 °C. What are the concentrations of A , B , and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? How would your answers change if the reaction had a standard free‑energy change of + 5.46...
A reaction A(aq) + B(aq) = C(aq) has a standard free-energy change of -3.06 kJ/mol at 25 °C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? How would your answers change if the reaction had a standard free-energy change of +3.06 kJ/mol? O There would be less A and B but more C. All concentrations would be higher. There...
A reaction A (aq) + B(aq) C(aq) has a standard free-energy change of-5.16 kJ/mol at 25 degree C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and 0 M, respectively? How would your answers above change if the reaction had a standard free-energy change of +5.16 kJ/mol? There would be less A and B but more C. All concentrations would be lower. All...
A reaction A(aq) + B(aq) = C(aq) has a standard free-energy change of -3.38 kJ/mol at 25°C. What are the concentrations of A, B, and C at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M, 0.40 M, and OM, respectively? [A] = [B] = 1C) = How would your answers change if the reaction had a standard free-energy change of +3.38 kJ/mol? There would be no change to the answers. O All concentrations would be...