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- Calculate the percentage change in Kx for the reaction H2CO(g) ⇋ CO(g) + H2(g) when the total pressure is increased from 1.0 bar to 2.0 bar at constant temperature.A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?The solubility product constant, Ksp, at 25°C for AgI(s) in water has the value 8.3 × 10–17. Calculate ΔG at 25°C for the process AgI(s) ⟷⟷ Ag+(aq) + I–(aq) where [Ag+] = 9.1 × 10–9 M and [I–] = 9.1 × 10–9 M. (R = 8.314 J/K • mol)
- Calculate the percentage change in Kx for the reaction CH3OH(g) + NOCl(g) ⇋ HCl(g) + CH3NO2(g) when the total pressure is increased from 1.0 bar to 2.0 bar at constant temperature.What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The conditions for this reaction are: PO2 = 1.75 bar PO3 = 1.99 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass. Please use the method of Gibbs energy of formation to calculate ΔrG° if needed. Enter the value of "Q" for this reaction.For the reaction S(s,rhombic) + 2co(g)----> so2(g) +2c(s, graphite) Delta H =75kj and delta s= -167.6j/k The equilibrium constant for this reaction at 298.0 k is ----- Assume that delta h and delta s are independent of temperature.
- The solubility product constant, Ksp, for barium sulfate, BaSO4, is 1.1 x 10-10. Compare the solubility of barium sulfate in water to its solubility in a 0.100 M solution of sodium sulfate. Support your comparison with calculations. Solubility in water: Solubility in sodium sulfate solution: Use significant figures!Calculate the partial pressure of PCl5 at 1.00 bar total pressure and 400 K: PCl3 + Cl2 ---> PCl5 The original reaction mixture contains 1.00 mol PCl3 and 2.00 mol Cl2. Let the Gibbs free energy change be -3533 J.Two students prepared aqueous solutions of LiCl and measured the properties, as shown in the table above. Both students observed that the solid LiCl readily dissolved in H2O. The students drew particle diagrams to explain the changes in the enthalpy and entropy of dissolution for LiCl based on their results and observations. Based on this information, the better particle diagram was drawn by which student, and why is that diagram more accurate? (see attached image) a.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+ and Cl− ions causing an increase in entropy. b.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+and Cl−ions indicating that the dissolution of LiCl is exothermic. c.) The better particle diagram was drawn by Student 2 because it shows that LiCl does not dissociate, resulting in a decrease in entropy for the dissolution of LiCl.…
- Calculate the value of ΔHm − ΔUm for the reaction N2(g) + 3 H2(g) → 2 NH3(g) at 298 K.At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.79 . If the concentration of B(aq) were 0.311 M and the concentration of C(aq) were 0.477 M, what would be the minimum concentration of A(aq) required (in mol/L) to make this reaction spontaneous under these conditions?Chemistry Using the information in the data section, calculate the standard reaction ent and standard reaction Gibbs energy for the n2(g)+3h2(g) → 2nh3(g) reaction.