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Please answer question 3 Part A and B
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- Math toolbox: ax2+bx+c =0 solve ; 1 cm3 = 0.001 dm3 The equilibrium constant is calculated Keq = 0.36 for the reaction @ 400 K when using M (mol/dm3) as the unit for the gasses. note: not the pressure unit. PCl5 (g) <=> PCl3 (g) + Cl2 (g) When using M as the units, the Keq is unitless with unit canceled to CѲ= 1 M. Giving that 5.365 g of PCl5 (Mw = 208 g/mol) was initially placed in a reaction vessel of volume V = 250 cm3. When reach equilibrium, determine the molar concentrations of PCl3 in the mixture assuming ideal gasses for all. concentration of PCl3 = ______ M. 3 sig. fig.A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show workA mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?
- 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=sharingIf the Ksp for the dissolution of barium phosphate is 6.00*10^-39 then what is the equilibrium concentration of barium cations in solution if excess barium phosphate is added to water? Give typing answer with explanation and conclusionOn 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.
- The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate unitsGiven the equation CH4 (g) + H2O (g) --> CO (g) + 3H2 (g). At 298K, take equilibrium constant K = 1.19x10^-25. At T=1004K, the equilibrium constant is 3.0. At 1004K, the initial partial pressure PCH4 = 30 atm, PH2O = 50 atm and equilibrium is reached at this temperature. After equilibrium is reached, what is the partial pressure and mole fraction of all components? please write correctly last time equation is not redable if possible write on paperOn 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 4.0 L vessel. What would the Equilibrium Contant, Kc, be in this equation?
- b) In a company that wants to use this gas equilibrium as a source of hydrogen gas H2, it is desired with a gas pressure of hydrogen equal to 7,850 atm. What equilibrium pressure in atm of ethanol C2H5OH is required to satisfy this requirement? c) What must the initial pressure of ethanol be to meet the requirement for 7,850 atm H2 gas at equilibrium? Supplied: Use an S E L table to organize data and set up the expression for Kc after Guldberg-Waages mass action law for the homogeneous gas equilibrium if possible, I would like handwritten answers with calculations. Thanks :)Determine the equilibrium constant (Kc): data is attached if neededHypothetical reaction A2 <--> A The In Kp = -33.47 at 2000K while deltaH0 = 205200 +4.94T - 0.888*10-3 T2 . At equilibrium, what will be the partial pressure of each component at a temperature of 8000K and 2atm total pressure?