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
- Sodium reacts violently with water according to the equation Na(s) + H2O() NaOH(aq) + H2(g) Without doing calculations, predict the signs of rH and rS for the reaction. Verify your prediction with a calculation.arrow_forwardCalculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.arrow_forwardNatural gas, which is mostly methane, CH4, is a resource that the United States has in abundance. In principle, ethane can be obtained from methane by the reaction 2CH4(g)C2H6(g)+H2(g) (a) Calculate G° at 25°C for the reaction. Comment on the feasibility of this reaction at 25°C. (b) Couple the reaction above with the formation of steam from the elements: H2(g)+12O2(g)H2O(g)G=228.6kJ What is the equation for the overall reaction? Comment on the feasibility of the overall reaction.arrow_forward
- For the following reactions at constant pressure, choose the correct relationship between AH and AE. 2HF(g) → H2(g) + F2(g) ΔΗ>ΔΕ ΔΗ ΔΕ Ο ΔΗ ΔΕ ΔΗ<ΔΕ ΔΗ-ΔΕ depends on the conditionsarrow_forwardConsider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)Mg(�)+Fe2+(��)→Mg2+(��)+Fe(�) at 73 ∘C∘C , where [Fe2+]=3.80mol L−1[Fe2+]=3.80mol L−1 and [Mg2+]=0.210mol L−1[Mg2+]=0.210mol L−1 . What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)Mg(�)+Fe2+(��)→Mg2+(��)+Fe(�) at 73 ∘C∘C when [Fe2+]=3.80mol L−1[Fe2+]=3.80mol L−1 and [Mg2+]=0.210mol L−1[Mg2+]=0.210mol L−1. Assume that the standard cell potential does not depend on temperature. Express your answer to three significant figures and include the appropriate units.arrow_forwardWhich of the following statements are TRUE?(1) Reactions with more negative values of △G0 are spontaneous and proceed at a higher rate than those with less negative values of △G0.(2) The activation energy, Ea, is usually about the same as △H for a reaction.(3) The activation energy for a reaction does not change significantly as temperature changes.(4) Reactions usually occur at faster rates at higher temperatures. (A) 1, 2, 3, 4 (B) 3, 4 (C) 1, 2, 4 (D) 2, 3, 4 (E) 1, 2, 3arrow_forward
- 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_forwardUnder what circumstances are ΔE and ΔH essentially equal? a) ΔV=0 (there are the same number of reactant and product gas molecules). b) the rate of the reaction is extremely high such that reactants are quickly depleted. c) the temperature is constant throughout the reaction. d) ΔP=0 (the sum of the partial pressures of the products is equal to that of the reactants).arrow_forwardCalculate ΔG in kJ•mol-1 at 298 K for the following reaction: 2 A(g) + B2(s) → 2 AB(g) ΔGo = 49 kJ•mol-1 under the following conditions: P(A) = 0.446 atm, P(AB) = 0.823 atm A certain reaction A → B has a rate constant of 4.7 x 10–2 M s-1 at 25°C. An experiment was run at this temperature where the initial concentration of A is 0.342 M. What is the half-life of the reaction in seconds? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)arrow_forward
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