What is Ecell at 25°C for the reaction Ca(s) | Ca2+(2.898 M) || Sn2+(0.137 M) | Sn(s)? Report your answer to the hundredths place and do not include units. Half-reaction E° (V) Ca2+ + 2e- → Ca(s) -2.87 Sn2+ + 2e- → Sn(s) -0.14
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What is Ecell at 25°C for the reaction Ca(s) | Ca2+(2.898 M) || Sn2+(0.137 M) | Sn(s)? Report your answer to the hundredths place and do not include units.
| Half-reaction | E° (V) |
| Ca2+ + 2e- → Ca(s) | -2.87 |
| Sn2+ + 2e- → Sn(s) | -0.14 |
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- Calculate the equilibrium constants Keqo for the following reactions, using the standard free energy changes given below. (Note: if your calculation produces an overflow error, give the answer as a power of e.)a) Glucose + 6O2 --> 6CO2 + 6H2O (–2,840 kJ/mol)b) ATP + H2O --> ADP + Pi (–30.5 kJ/mol)c) Ethyl Acetate + H2O --> Ethanol + Acetate (+19.6 kJ/mol)The equilibrium constant for a chemical reaction was found to depend on temperature over the temperature range 400 K to 600 K according to the following equation:ln K(T) = A +BT+CT2where A, B, and C are the constants A = −3.53, B = −2736 K, and C = 2.2 × 105 K2.Calculate the standard reaction enthalpy and the standard reaction entropy at T =500 K.Calcium oxide (CaO), also called quicklime is prepared by decomposing limestone (CaCO3) in a kiln at high temperature and the reaction proceeds as: CaCO3 (s) CaO (s) + CO2 (g) Given : At T= 25 °C, then T=298 K AH° +177.8 kJ/mol AS° +160.5 J/K mol Calculate Gibbs Free Energy change (AG) for the reaction. -130.0 kJ/mol -160.5 kJ/mol +130.0 kJ/mol +160.5 kJ/mol
- A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = JDevelop a general equation for the standard heat of reaction as a function of temperature for one of the reactions given in parts (a), (b) a. C6H5C2H5(g) → C6H5CH:CH2(g) + H2(g) b. C(s) + H2O(l) → H2(g) + CO(g)Calculate ΔG∘ for the reaction 2H2O(l)⇌H3O+(aq)+OH−(aq). At 25 ∘C, Kw for the dissociation of water is 1.0×10−14.
- The standard Gibbs free energy change is 2.60 kJ/mol for the reaction at 25.0oC: H2(g) + I2(g) →← 2HI(g); ∆Gorxn = + 2.60 kJ/mol The reaction starts with equal molar amounts of H2(g) and I2(g) in a previously evacuated, constant volume vessel. What is the equilibrium mole fraction of HI? Enter your answers with correct units and significant figures.of 16 For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) = 2NH₂(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH, = 0.750 atm? AG = kJ/mol.What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous? what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean? If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system
- Consider the combustion of liquid methanol, CH3OH(l):CH3OH(l) + 3/2O2(g)----> CO2(g) + 2 H2O(l) ΔH = -726.5 kJ(a) What is the enthalpy change for the reverse reaction?(b) Balance the forward reaction with whole-number coefficients.What is ΔH for the reaction represented by thisequation? (c) Which is more likely to be thermodynamicallyfavored, the forward reaction or the reverse reaction?(d) If the reaction were written to produce H2O(g) insteadof H2O(l), would you expect the magnitude of ΔH to increase,decrease, or stay the same? Explain.Titanium can be produced by electrolytic reduction from an anhydrous molten salt electrolyte that contains titanium(IV) chloride and a spectator salt that furnishes ions to make the electrolyte conduct electricity. The stan- dard enthalpy of formation of TiCl4(liquid) is -750 kJ mol^-1, and the standard entropies of TiCl4(liquid), Ti(s), and Cl2(g) are 253, 30, and 223 J K^-1 mol^-1, respectively. What minimum applied voltage will be necessary at 100°C?Calculate ΔH°298 for the process Zn(s) + S(s) + 2O2(g)⟶ZnSO4(s)from the following information:Zn(s) + S(s)⟶ZnS(s) ΔH°298 = −206.0 kJZnS(s) + 2O2(g)⟶ZnSO4(s) ΔH°298 = −776.8 kJ