Predict the order of the following reactions in terms of increasing ΔS:
(a)
(c)
(d)
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Chemistry: Principles and Reactions
- Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.arrow_forwardMonochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.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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- Reaction at 25.0oC CO(g) + NO(g) → CO2(g) + N2(g) starts with the following initial partial pressures: (PCO2)0 = 0.50 atm, (PN2)0= 0.60 atm, (PCO)0= 5.0×10–35 atm, and (PNO)0 = 5.×10-36 atm. Substance ∆Gof, kJ mol CO2(g) – 394.4 N2(g) 0 CO(g) – 137.3 NO(g) + 86.7 Use the attached standard Gibbs free energies of formation to calculate: (a) KP for the reaction, (b) the immediate Gibbs free energy change for the reaction, ∆Grxn, and (c) check the correct box predicting the direction in which reaction proceeds. Enter your answers with correct units and significant figures, and check the correct box below: Reaction proceeds spontaneously forward towards equilibrium. Reaction is at equilibrium. Reaction proceeds spontaneously backward towards equilibrium.arrow_forwardPredict the effect of decreasingthe temperature on theamounts of reactants in the following reactions:arrow_forwardChemical reaction. Use data to Answer.arrow_forward
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