Example 10.3-2 Ethane is dehydrogenated to ethylene and acetylene in the following pair of catalytic reactions: C₂H6C₂H + H₂ C₂H6C₂H₂ + 2H₂ The reactions take place at 1 atm and proceed to a point such that the product gas composition satisfies the following equilibrium conditions: YC₂H₁ Y H₂= 3.75 YC₂H6 YC₂H₂ Yuz YC₂H6 = 0.135 Where y, is mole fraction. The product gas goes to a separation process that separates 95% of the unreacted ethane and recycles to the reactor, and ethane feed to the reactor is 100 mol/s. a) Set up the equations for all unknown stream variables,

Example 10.3-2 Ethane is dehydrogenated to ethylene and acetylene in the following pair of catalytic reactions: C₂H6C₂H + H₂ C₂H6C₂H₂ + 2H₂ The reactions take place at 1 atm and proceed to a point such that the product gas composition satisfies the following equilibrium conditions: YC₂H₁ Y H₂= 3.75 YC₂H6 YC₂H₂ Yuz YC₂H6 = 0.135 Where y, is mole fraction. The product gas goes to a separation process that separates 95% of the unreacted ethane and recycles to the reactor, and ethane feed to the reactor is 100 mol/s. a) Set up the equations for all unknown stream variables,

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)
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Identify the proper form of the equilibrium-constant expression for the equation N2 (g) + O2 (g) = 2NO(g) • View Available Hint(s) [NO] Ο Κ: [N2][O2] [NO]? O K: [N2][O2] 12 [N2][O2] O K = [NO]? 2[NO] Ο Κ- [N2][O2]
1.3 3 (i) In the Haber process for the production of ammonia, the following reaction occurs: 2 (g) + 3H₂(g) 2NH3(g) = DH is negative If the equilibrium concentrations for all the reactants and products at 600°C are: [N₂] = 0.40 mol/dm³, [H₂] = 1.20 mol/dm³ and [NH₂] = 0.20 mol/dm³ Construct an expression for K and calculate the numerical value of the equilibrium constant, K с (ii) At 500°C K. 0.062 mol 2dm. Compare this value to the one you calculated in 3(i) above and state whether the yield of ammonia is greater at 500°C or 600°C and briefly explain your choice.
Consider the following reaction: SO2Cl2 (g) SO2 (g) + Cl2 (g) A reaction mixture is made containing an initial [SO₂Cl₂] of 2.2x10-2 M. At equilibrium, [C1₂] = 1.1x10-² M. Calculate the value of the equilibrium constant (Kc). Express your answer using two significant figures. ΓΙ ΑΣΦ Kc = Submit Request Answer ?
At a certain temperature, the equilibrium constant K for the following reaction is 734.: NO3(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. ?
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4. What will be the effect of the following change on the given equilibrium system? system change result CH3OH is added to CH(g) +H20() =CH;OH(1) +H2(g) reaction container H2(g) + I2(g) = 2HI(g) an inert gas is added 2H2 (g) + O2 (g) = 2H20 (g) AH = -483.6 kJ/mol of O2 increase in temperature SnO2(g) + 2C(s) = Sn(s) + 2CO2(g) AH = + 360.0 KJ Pressure is decreased N2(g) + 3 H2(g) =2 NH3(g) AH = -92 kJ mol- the solution is cooled some AgNO; is added to the solution AgCl(s) = Ag*(ag) + CF(ag) N2(g) + 3 H2(g) =2 NH3(g) pressure is increased
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
Keq for a Gas-Phase Reaction A 5.00-L vessel contained 9.49×102 mol of gaseous PCI3, 8.03×102 mol of gaseous PCI5, and 8.21x102 mol of Cl2 gas at equilibrium at 233°C. Calculate the value of Keg (expressed in terms of the molar concentrations) for the reaction PCI3(g) + Cl2(g) = PCI5(g) (No units required.)
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