If K = 1.25x10® & the initial concentrations of A & B are0.100 M, calculate the equilibrium concentrations ofA, B and C:A + B 2 Cboju ou bLOcoeg co buognc o uacpumsq no tnlogerh montOL LOUCISUeSboiq of bsasoiq no Inlog 1er mot noilase ori liwcousmil i6SC K-10X1

Answered: Image /qna-images/answer/c0342599-38bd-4f13-b292-54cc3a8e0339.jpg

If K = 1.25x10 & the initial concentrations of A & B are 0.100 M, calculate the equilibrium concentrations of A, B and C: A + B 2 C rh mot noitosm orti liw 0 M0010.0 bris 8 M 00A 0 o1s 19mit is en boju ou bLOCoeq co buoqnc o acpun of baas01g no lnlog 1sr moit noilose orl 6016Gmi t6 enoilsneonO OL LOUCISU(23

If K = 1.25x10 & the initial concentrations of A & B are 0.100 M, calculate the equilibrium concentrations of A, B and C: A + B 2 C rh mot noitosm orti liw 0 M0010.0 bris 8 M 00A 0 o1s 19mit is en boju ou bLOCoeq co buoqnc o acpun of baas01g no lnlog 1sr moit noilose orl 6016Gmi t6 enoilsneonO OL LOUCISU(23

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...

See similar textbooks

Similar questions

At particular temperature, 5.2 moles of A is placed into 1.0 L container and A dissociate by the reaction 2A(g) 2B(g) +C(g). (---> is equilbrium sign) ---> At equilibrium the concentration of B(g) is 2.0 M. Calculate K for this reaction a. 0.39 b. 0.29 c. 0.78 d. 0.23 e. 0.10
In the fictitious reaction below, the equilibrium concentration of A is 0.7140 M, B is 0.1133 M, and A 2B 3 is 0.5984 M. What is the value of the equilbrium constant k for this reaction? 2 A (ag) + 3 В (aq) А 2B з 0.001239 128.1 8.778 7.397 807.1
الطريقة ساوصحها Q) 0.5 M each of H2 and I2 are introduced into a sealed flask The following reaction occurs until equilibrium is established. Calculate the equilibrium concentrations of H2, 1, and HI. Kc = 50.5 Hz18) 218) 2 2Hl(g) Solution : AR Ai di M arch Ps
4. For the system below you start with 0.6 moles of NOCI in a 1.5 L container and the K, value is 1.56 x 106 determine all the equilibrium concentrations. 2NOCI(g) 2NO(g) + Cl₂(g) OC €
9 O search X What is the expression for the equilibrium constant? SO₂(g) + ¹/2O2(g)SO3(g) о a) Keg E Ob) Keg Od Keq - O d) Keg C R = 6: Ps03 Pso2 P2 Ps03 P³ 02 Ps02 02 Ps03 Pso₂ Po₂ Ps03 Pso₂ P1/202 T G B H ARUD $ S 41 8 00 N J C - K M 11
P Question // Q 10) Find the value of the equilibrium constant expression. Fe3+ SCN- FESCN2+ 1.3 x 10-3 1.3 x 10-3 C -1.80 x 10-4 -1.80 x 10-4 +1.80 x 10-4 1.1 x 10-3 1.1 x 10-3 +1.80 x 10-4
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
What is the equilibrium expression for the following reaction? CH(8) + 20,(g) = CO:(g) + 2H;0(g) [co.JH,0] TCH 0] A K= [co.JH,0) TCH.Jo.F [co.HH,0] [CH Ho.] C K=- D Not applicable
The equilibrium constant, K, for the following reaction is 7.00x10 at 673 K. NH,IG) NH,(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.254 mol NH,I, 8.37x10 M NH and 8.37x10 M HI. If the concentration of HI() is suddenly increased to 1.20x10² M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH]= [HI]
lab2-1: please see attached
How can find what k= ?
A mixture initially contains AA, BB, and CC in the following concentrations: [A][A]A_1 = 0.700 MM , [B][B]B_1 = 1.15 MM , and [C][C]C_1 = 0.300 MM . The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A][A]A_2 = 0.570 MM and [C][C]C_2 = 0.430 MM . Calculate the value of the equilibrium constant, KcKcK_c.