At 700 K, the reaction 2502(9) + O2(9) = 2503(9) has the equilibrium constant Ke = 4.3 x 106, and the following concentrations are present: [SO2) = 0.010 M: [SO3) = 10. M: [02) = 0.010 M. Which of the following is true based on the above? Multiple Cholce Qc < Kc. the reaction proceeds from right to left to reach equilibrium Qc- Kc, the reaction is currently at equilibrium Q> Kc. the reaction proceeds from right to left to reach equilibrium Qc < Kc. the reaction proceeds from left to right to reach equilibrium Qc> Ke, the reaction proceeds from left to right to reach equilorium

At 700 K, the reaction 2502(9) + O2(9) = 2503(9) has the equilibrium constant Ke = 4.3 x 106, and the following concentrations are present: [SO2) = 0.010 M: [SO3) = 10. M: [02) = 0.010 M. Which of the following is true based on the above? Multiple Cholce Qc < Kc. the reaction proceeds from right to left to reach equilibrium Qc- Kc, the reaction is currently at equilibrium Q> Kc. the reaction proceeds from right to left to reach equilibrium Qc < Kc. the reaction proceeds from left to right to reach equilibrium Qc> Ke, the reaction proceeds from left to right to reach equilorium

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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Gaseous hydrogen iodide is placed in a closed containerat 425 °C, where it partially decomposes to hydrogen andiodine: 2 HI1g2 ∆ H21g2 + I21g2. At equilibrium it isfound that 3HI4 = 3.53 * 10-3 M, 3H24 = 4.79 * 10-4 M,and 3I24 = 4.79 * 10-4 M. What is the value of Kc at thistemperature?
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The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCI3(g) + Cl₂(g) =PC15(9) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of PCI3 and 0.451 moles of Cl₂ are introduced into a 1.00 L vessel at 500 K. [PCI3] = [Cl₂] [PCI5] = = ΣΣΣ
PCI, (g) = PCI; (g)+ Cl, (g) @ 500 Kelvin K, = 0.497 In an equilibrium mixture at 500 K, PPCI5 = 0.860 atm and P = 0.350 atm. What is Pep in the equilibrium PC13 C12 mixture?
Q=1.45 12b
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Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH; CO,H + C,H OH = CH; CO,C,H; + H20 K = 2.2 Acetic acid Ethanol Ethyl acetate For the following mixtures (a-d), will the concentration of H2 O increase, decrease, or remain the same as equilibrium is established? а. [сH,CO,C, Ны] — 0.22 М, [Н,0] — 0.1о м, [сH,СО, н] — 0.010 м, [C, H, онј — 0.010 M O increase O ecrease O remain the same b. [CH; CO2C,H5] = 0.22 M, [H2O] = 0.0020 M, [CH3 CO,H] = 0.0020 M, [C,H;OH] = 0.10 M O increase O decrease Oremain the same c. [CH; CO2C,H5]= 0.88 M , [H2O] = 0.12 M, [CH; CO,H] = 0.044 M, [C,H; OH] = 6.0 M с. O increase decrease Oremain the same d. [CH3 CO,C,H5]= 4.4 M , [H2O] = 4.4 M, [CH3 CO,H] = 0.88 M , [C,H5 OH] = 10.0 M O increase O decrease Oremain the same e. What must the concentration of water be for a mixture with [CH3CO,C,H5] = 1.0 M, [CH3 CO;H] = 0.10 M , and [C2H; OH] = 6.0 M to be at equilibrium? Concentration м
Consider the reaction: N₂O4 (9) — 2NO2 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: N₂(g) +202 (g) = N₂O4 (9) K₁ 1/2N₂(g) + O2(g) — NO2(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter Kif the first equilibrium constant should be squared. K=
41
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Ammonia can be synthesized according to the reaction: N2(g) + 3H2(g) = 2NH3(g), K = 5.3x10-5 at 725K. A 200.0L reaction container intially contains 1.27kg of N2 and 0.310kg of H2 at 725K. Assuming ideal gas behaviour, calculate the mass of NH3 (in g) present in the reaction at equilibrium. What is the percent yield under these conditions?
Be sure to answer all parts. The equilibrium constant K, for the reaction H2(g) + I2(g) =2 HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H,, I,, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0.222 M and [HI] = 0 M. (H2leq = |0.0692 [Lleg =|0.182 [HI]eg =0.826 < Prev 18 of Microsoft Store