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- PLEASE GO THROUGH AND HELP ME. -the concentration of standard sodium thiosulphate solution is 0.01152 M. -the temperature of the equilibrium mixture in degree Celsius is 20oC. In Determination #1: Volume of thiosulphate = 32.50 mL Volume of Aqueous aliquot = 10.15 mL Strength of Thiosulphate = 0.01152 M In Determination #2: Volume of thiosulphate = 32.50 mL Volume of Aqueous aliquot = 10.23 mL Strength of Thiosulphate = 0.01152 M In Determination #3: Volume of thiosulphate = 32.67 mL Volume of Aqueous aliquot = 10.31 mL Strength of Thiosulphate = 0.01152 M https://drive.google.com/file/d/1824fGKn1AMdByzDsSLq8Nv323rpC4e79/view?usp=sharingManipulate the equilibrium constant to reflect changes in thechemical equation?In the contact process: DH = -197 kJ mol-1 Predict the position of equilibrium when: both the temperature and pressure are decreased
- What is the equilibrium constant for a reaction at temperature 59.3 °C if the equilibrium constant at 25.7 °C is 30.3? Express your answer to at least two significant figures. For this reaction, ΔrH° = -4.2 kJ mol-1.For a certain reaction, Kc�� = 9.80×10−10 and kf=�f= 2.59×10−5 M−2⋅s−1�−2⋅s−1 . Calculate the value of the reverse rate constant, kr�r, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s) For a different reaction, Kc�� = 5.40×102, kf=8.96×103s−1�f=8.96×103s−1 , and kr=�r= 16.6 s−1s−1 . Adding a catalyst increases the forward rate constant to 2.05×106 s−1s−1 . What is the new value of the reverse reaction constant, kr�r, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1�−2⋅�−1 include ⋅⋅ (multiplication dot) between each measurement. View Available Hint(s)Consider the mixing of 25.00 mL of 0.0500 M Pb(NO3)2 with 25.00 mL of 0.0500 M NaCl and the equilibrium reaction, PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq) Ksp = 1.20 x 10-5 What is the molar concentration of Pb2+ in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the molar concentration of Cl- in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the ion product (Q)? Will a precipitate form? (yes or no)
- Given the equation of reaction for methanol and is in equilibrium within a fixed volume tank.The direct reaction is exothermic. CO(g) + 2H2(g) ⇄ CH3OH(g) 1. a. Write down the phrase to establish equilibrium b. Calculate the equilibrium constant of the reaction when the following data were obtained afterReaching equilibrium at room temperature: [CO]= 6.0×10-2 M[H2] = 1.0×10-2 M[CH3OH] = 3.5×10-4 M 2. This reaction is as stated exothermic. Despite this you heat up at the beginning of the processThe gas mixture. Why is it advisable to heat the reaction tank? 3. Write how the quantity of the product will be affected when one of the following disturbances occurs after arrivalFor the equilibrium state:1. Cool the reaction vessel.2. Reduce the volume of the reaction vessel.3. Add a catalyst to the system.Explain your answers in each section. 4, . Will there be an increase or decrease in entropy during the direct response recorded above? Necrosis. 5. What is the sign of delta Go In the…Zn Zn2+(1.0M) Cu2+ (1.00M) Cu Ecell, reaction quotient, Eºcelli think it is The reaction quotient can be calculated from the reactants' and products' concentrations or partial pressures. 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) At non-standard conditions, the concentrations are: [SmCl3] = 2.00 M [Li] = 2.00M [Sm] = 0 (solid) [LiCl] = 0.0100 M The reaction quotient (Q) can be calculated as follows: Q = {[LiCl]^6}/[Sm3+ ]^2[Cl3]^2 = (0.0100)^6 /(2.00)^2 x (2.00)^2 = 6.25 x 10^-14
- Calculate the concentration equilibrium constant KC at 298 K for the reaction N2O4 (g) = 2 NO2 (g) if at this temperature the pressure equilibrium constant is 0.146 bar for the reaction. Answer: [5.89 x 10-3 mol dm-3 ]On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) + S2(g)was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0L vessel.Calculate the equilibrium constant, Kc, for this reaction.Equal quantities of 0.010M0.010M solutions of an acid HAHA and a base BB are mixed. The pHpH of the resulting solution is 9.4. Write the equilibrium equation for the reaction between HAand B. Express your answer as a chemical equation. Identify all of the phases in your answer. If Ka for HA is 9.0×10−5, what is the value of the equilibrium constant for the reaction between HA and B? Express your answer using one significant figure. Keq= What is the value of Kb for B? Express your answer using one significant figure. Kb=