Consider the following... CO2(g) + CF4(g) = 2COF2(g) K= 0.50 In a reaction container the initial concentrations are... [CO2] = 0.50 M, [CF4] = 0.50 M, [COF2] = 0.30 M %3D To reach equilibrium, the reaction will proceed_. a. left since Q < K b. left since Q > K c. right since Q < K d. right since Q > K

Consider the following... CO2(g) + CF4(g) = 2COF2(g) K= 0.50 In a reaction container the initial concentrations are... [CO2] = 0.50 M, [CF4] = 0.50 M, [COF2] = 0.30 M %3D To reach equilibrium, the reaction will proceed_. a. left since Q < K b. left since Q > K c. right since Q < K d. right since Q > K

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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Booking.com: Chea.. TripAdvisor Facebook [References] The reaction 2 NO2(s) N20.(g) has an equilibrium constant, K. of 170 at 25 °C. If 4.5 x 10 mol of NO2 is present in 10.-L flask along with 3.5 x 10 mol of N204, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds to equilibrium? The system is V. The concentration of NO2 will Vas the system proceeds to equilibrium. Submit Answer Try Another Version 2 Item attempts remalning Previous Email Instructor Save and Exit ment Ceneare Learning Ceneae A
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Consider the equilibrium reaction and its equilibrium constant expression. [ICI]? 1(g) + Cl,(g) 2 2ICI(g) K = L] C] For the reaction 2ICI(g) = 1(g) + Cl,(g) select the equilibrium constant expression. K' О к [ICI]4 2|ICÍ] [L] [CL] L][Cl] [ICI]? [ICi]* K': K' = [Ici]? K' %3D L][CL]
10. A mixture of CO and Cl, is placed in a reaction flask that is then sealed. Initially (CO) = 0.0102 mol/L and (Cl,) = 0.00609 mol/L. When the reaction %3D CO(g) + Cl,(g) COCI,(g) reaches equilibrium at 600 K. [CI,] = 0.00301 mol/L. a) Calculate the concentrations of CO and COCI, at equilibrium. b) Calculate K.
The equilibrium constant, K. for the following reaction is 7.00x10-$ at 673 K. NH,I(3)ENH3(3) + HI(E) Calculate the equilibrium concentration of HI when 0.521 moles of NH,I(s) are introduced into a 1.00 L vessel at 673 K. [HI] = M
5. The equilibrium constant expression of a gas reaction is [CS2] [H2]* _ [CH4] [H2S]? K. Write the balanced chemical equation corresponding to this expression
The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl(g) COCI,(g) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of CO and 0.451 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] [Cl] [COCL,] = MMM
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Chemical Equilibrium A. Write the K formula for the following reactions. 1. 3NO(g) → N2O(g) + NO2(g) 2. CH4(g) + 2H2S(g) → CS2(g) + 4H2(g) 3. Ni(CO)4(g) → Ni(s) + 4CO(g) 4. Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g) 5. 2N205(g) → 4NO2(g) + O2(g)
At equilibrium, the concentrations in this system were found to be [N,] = [O,] = 0.200 M and [NO] = 0.500 M. N2(g) + O2(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NO]inal M
A 1.00 liter flask contained 0.24 mol NO2 at 700 K which decomposed according to the reaction 2 NO2(g) = 2NO(g) + O2(g). At equilibrium the amount of NO was measured to be 0.14 mol, what is the value of Kc? A. 9,6 x 103 B. 1.1 x 102 C. 9.8 x 102 D. 1,4 x 101 E. 5.7 x 103
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