Kindly answer 1-7. Thank you! Much appreciated 1.) Given the reaction: 2 H2S(g) =2 H2(g) + S2(g)If Kp = 0.012, what should be the initial pressure of pure H2S to produce an equilibrated mixturecontaining 0.250 atm of H2 (g)?2.) Given the reaction: 3H2(g) + N{g) = 2NH(g}Calculate the Kp if Kc is 0.105 at 472°C.Use the formula: Kp = K.(RT)An (where R=0.0821, An= moles products – moles reactants)3.) Given the reaction: CO2(g) + H2(g) = H2O(g)+ CO(g)If Kc = 1.6 at 1263 K, calculate the number of moles of carbon monoxide gas (CO) in the finalequilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O,and 1.00 mol of CO to a 5.00 L reactor at the given temperature.4.) Given the reaction: PCI3(g) + Cl2(g) = PCI5(g)Kc = 24.3Suppose the system at that particular temperature is prepared with [PCI3] = 0.10 M, [Cl2] = 0.15 M,and [PCI5} = 0.55 M. Is the reaction at equilibrium? If not, determine whether it will shift to the left orright to reach equilibrium.5.) What CrO,2 concentration is required to initiate precipitation of Ag2CrO4 from a solution that is0.0125 M in Ag*? (Ksp= 1.2 x 10-12)6.) Given the following information:2 A(g) + B(g) = A2B(g)2 A(g) + C2(g) =2 AC(g)K1 = 5.0 x 10*K2 = 3.2 x 103What is the net equilibrium constant (Knet) for the reaction?2AC(g) + 4A(g) + 3B(g) = 3 AB(g} + C{g}7.) Given: Solubility product for a series of hydroxides:Kp = 4.0 x 10-10 = [BiO*][OH]Ksp = 7.0 x 10-22Ksp = 3.0 x 10-24BIOOHBe(OH)2Tm(OH)3(a) Which hydroxide has the lowest molar solubility in water?(b) Which hydroxide has the highest molar solubility in a 0.10 M NaOH solution?

1.) Given the reaction: 2 H2S(g)=2 H2(g) + S2(g) If Kp 0.012, what should be the initial pressure of pure H2S to produce an equilibrated mixture containing 0.250 atm of H2 (g)? 2.) Given the reaction: 3H2(g) + Ng)=2NH(g) Calculate the Kp if Kc is 0.105 at 472°C. Use the formula: Kp K.(RT)An (where R-0.0821, An= moles products- moles reactants) 3.) Given the reaction: CO2(g) + H2(g) H20(g) + CO(g) If Kc = 1.6 at 1263 K, calculate the number of moles of carbon monoxide gas (CO) in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of COn, 0.750 mol of HO, and 1.00 mol of CO to a 5.00L reactor at the given temperature.

1.) Given the reaction: 2 H2S(g)=2 H2(g) + S2(g) If Kp 0.012, what should be the initial pressure of pure H2S to produce an equilibrated mixture containing 0.250 atm of H2 (g)? 2.) Given the reaction: 3H2(g) + Ng)=2NH(g) Calculate the Kp if Kc is 0.105 at 472°C. Use the formula: Kp K.(RT)An (where R-0.0821, An= moles products- moles reactants) 3.) Given the reaction: CO2(g) + H2(g) H20(g) + CO(g) If Kc = 1.6 at 1263 K, calculate the number of moles of carbon monoxide gas (CO) in the final equilibrium system obtained by initially adding 1.00 mol of H2, 2.00 mol of COn, 0.750 mol of HO, and 1.00 mol of CO to a 5.00L reactor at the given temperature.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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