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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
For the equilibrium, Co2+(aq)+4SCN-(aq)⇄Co(SCN)2-(aq), K=1.0x103. Which of the following conditions are at equilibrium?
[Co2+]=1.1 M, [SCN-]=0.13 M, [Co(SCN)2-]=2.4x10-4M | |
[Co2+]=1.2 M, [SCN-]=0.050 M, [Co(SCN)2-]=7.5x10-3M | |
[Co2+]=0.75 M, [SCN-]=0.064 M, [Co(SCN)2-]=0.18 M | |
[Co2+]=0.010 M, [SCN-]=0.0010 M, [Co(SCN)2-]=0.10 M |
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- The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K. Calculate K. for this reaction at this temperature. NH4I(s) =NH3(g) + HI(g) Kcarrow_forwardhelparrow_forwardGiven these initial concentrations: [SCN] = 0.000646 M, [Fe³+] = 0.000506 M, and [Fe(SCN)²+] = 0.000000 M, determine The value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M. value for K: 1.09 X10-4 Incorrectarrow_forward
- Calculate the equilibrium concentration of Cu2+in a solution initially with 0.050 M Cu(NH3)42+ and 1.00 M NH3 given the equilibrium: Cu(NH3)42+(aq) ↔ Cu2+(aq) + 4NH3(aq) where Kd = 5.9 x 10-14. 7.2x10-15M 5.4x10-8M 1.1x10-17M 2.9x10-14Marrow_forwardAt 37.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has K = 2.94x10-8. If [H2O] = 55.5 mol L-1, [H+] = 95.4 µmol L-1, and [HCO3-] = 12.4 mmol L-1 at equilibrium, determine the PCO2 (pressure of CO2) in bar.arrow_forwardGiven these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.arrow_forward
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