For the decomposition of Ag2O: 2Ag2O(s)-4Ag(s)+O2(g) (a) Obtain an expression for AG° as a function of temperature. Prepare a table of AG° values at 100 K intervals between 100 K and 500 K. (b) Calculate the temperature at which AG°= 0.
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- What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)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.The value of the equilibrium constant at 25ºC, corresponding to the reaction: 3 C2H2 (g) = C6H6 (g), is Keq = 1.22 Taking into account this information, indicate V or F as appropriate,Justify:I) The Gibbs free energy of this reaction is = 0II) The Gibbs free energy of this reaction is <0III) The reaction is spontaneous to the rightIV) It is advisable to manufacture benzene under these conditions.a) TFTF b) TTTT c) FFTT d) FTTT e) FTFT f) TFTT g) TFFF
- 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/molThe value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.At 25 ∘C25 ∘C, the equilibrium partial pressures for the reaction A(g)+2B(g)↽−−⇀C(g)+D(g) were found to be ?A=4.34PA=4.34 atm, ?B=4.47PB=4.47 atm, ?C=6.00PC=6.00 atm, and ?D=5.45PD=5.45 atm. What is the standard change in Gibbs free energy of this reaction at 25 ∘C25 ∘C?
- Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation (∆Gof) of NH3 (g) is -105 kJ/mol at 304 K, calculate the equilibrium constant, K, at this temperature.To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3. K =Consider the (endothermic) thermal decomposition of calcium carbonate:CaCO3(?) → CaO(?) + CO2(?). For this reaction, ∆rH° = +178 kJ/moland ∆rS° =+161 JmolK. Determine the decomposition temperature, which is the temperature for which the equilibrium constant becomes greater than 1.1. Given the following data at standard conditions (all pressures equal to 1 atmatm and the common reference temperature 298 KK), what is the value of KpKpK_p for this reaction?
- What is the change in entropy when one mole of calcite (CaCO3) decomposes at 298.2 K to CaO(s)and CO2(g)?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.The equilibrium constant of a reaction is found according to the expression In K A + B / T + C / T3. between 400 K and 500 K where A = -2.04, B = -1176 K, and C = 2.1 x 107 'K3 Calculate the enthalpy of the standard reaction and the entropy of the standard reaction at 450 k. Calculate and explain their chemical analysis