(a)
Interpretation: It is to be shown that,
Concept introduction:
To show: At equilibrium,
(b)
Interpretation: It is to be shown that,
Concept introduction:
To show: At equilibrium,
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Chemistry: An Atoms First Approach
- For the reaction:2H2(g) + O2(g) ------> 2H2O(l) Calculate ΔS°sys _____J/K Calculate ΔS°surr _____ J/Karrow_forwardIn glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?arrow_forwardA chemist fills a reaction vessel with 0.419 g calcium phosphate Ca3PO42 solid, 0.388 M calcium Ca+2 aqueous solution, and 0.526 M phosphate PO4−3 aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy ΔG for the following chemical reaction: Ca3PO42s+3Ca+2aq2PO4−3aq Round your answer to the nearest kilojoule.arrow_forward
- A reaction Occuring in a Star 2 b 3 c H + H---> He + n a 1 2 d In order to balance the equation above, the values of a,b,c,d arearrow_forwardConsider the following reaction with equilibrium constant 0.02532 at 25 oC. 2 A (g) + B (g) -------- 3 C(g) Determine free energy change for a mixture of 0.75 mol A, 1.20 mol C and 3.40 mol B in a 5.0-L vessel at 25 oC considering the above reaction in forward direction.arrow_forwardFor the reaction 2NO(g)+ 2H2(g)-> N2(g)+2H2O(l) Delta H° = -752.2kj and delta S°= -351.6J/K The standard free energy change for the reaction of 2.08 moles of NO(g) at 286K, 1atm would be .......KJ. This reaction is reactant/product-favored under standard conditions at 268 K. Assume that Delta H and delta S are independent of temperature. Fill in the blank and choose what type of reaction this is.arrow_forward
- 2b) Which of these, the activation energy or the net free energy change, determines whether a reaction is chemically defined as "spontaneous"?arrow_forwardreaction A(aq)+B(aq)↽−−⇀C(aq)A(aq)+B(aq)↽−−⇀C(aq) has a standard free‑energy change of −3.47 kJ/mol−3.47 kJ/mol at 25 °C.25 °C. What are the concentrations of A,A, B,B, and CC at equilibrium if, at the beginning of the reaction, their concentrations are 0.30 M,0.30 M, 0.40 M,0.40 M, and 0 M,0 M, respectively? [A]=[A]= MM [B]=[B]= MM [C]=[C]= MM How would your answers change if the reaction had a standard free‑energy change of +3.47 kJ/mol?+3.47 kJ/mol? There would be no change to the answers. All concentrations would be lower. There would be less AA and BB but more C.C. There would be more AA and BB but less C.C. All concentrations would be higher.arrow_forwardConsider the reaction 2O(g)=O2(g) a. Predict deltaH and deltaS. b. Would the reaction be more spontaneous at high or low temperatures?arrow_forward
- For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard free enthalpy variation is 1.43 kJ at 25oC. The initial concentration of A is 0.541 M, the initial concentration of B is 0.343 M, and the initial concentration of C is 0.267 M. At equilibrium (we are still at 25oC), what will be the concentration of A( aq) (in mol/L)?arrow_forwardA reaction A(aq)+B(aq)↽−−⇀C(aq) A ( aq ) + B ( aq ) ↽ − − ⇀ C ( aq ) has a standard free‑energy change of −3.71 kJ/mol − 3.71 kJ / mol at 25 °C. 25 °C. What are the concentrations of A, A , B, B , and C 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 +3.71 kJ/mol? - There would be more A and B but less C.There would be less A and B but more C. - All concentrations would be lower. - There would be no change to the answers. - All concentrations would be higher.arrow_forwardCobalt(II) chloride hexahydrate, CoCl26H2O, is a bright pink compound, but in the presence of very dry air it loses water vapor to the air to produce the light blue anhydrous salt CoCl2. Calculate the standard free-energy change for the reaction at 25C: CoCl26H2O(s)CoCl2(s)+6H2O(g) Here are some thermodynamic data at 25C: What is the partial pressure of water vapor in equilibrium with the anhydrous salt and the hexahydrate at 25C? (Give the value in mmHg.) What is the relative humidity of air that has this partial pressure of water? The relative humidity of a sample of air is Relativehumidity=partialpressureofH2O(g)inairvaporpressureofwater100 What do you expect to happen to the equilibrium partial pressure over the hexahydrate as the temperature is raised? Explain.arrow_forward
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