When 15.0 mL of a8.80 x 105 M ammonium carbonate solution is combined with 12.0 mL of a5.71 x 10 M nickel(II) bromide solution does a precipitate form? (Kp (NiCO₂) = 6.6 × 10-)OYes, the precipitate forms.No, the precipitate doesn't form.For these conditions the Reaction Quotient, Q, is equal toSubmit Answer

We know if the Ionic product is more than solubility product then precipitate forms.If ionic product…

When 15.0 mL of a 8.80 x 105 M ammonium carbonate solution is combined with 12.0 mL of a 5.71 x 10 M nickel(II) bromide solution does a precipitate form? ( Kp (NiCO3) = 6.6 × 10-) OYes, the precipitate forms. No, the precipitate doesn't form. For these conditions the Reaction Quotient, Q. is equal to Submit Answer

When 15.0 mL of a 8.80 x 105 M ammonium carbonate solution is combined with 12.0 mL of a 5.71 x 10 M nickel(II) bromide solution does a precipitate form? ( Kp (NiCO3) = 6.6 × 10-) OYes, the precipitate forms. No, the precipitate doesn't form. For these conditions the Reaction Quotient, Q. is equal to Submit Answer

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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For the following reaction, Kc CO (g) + Cl₂ (g) = COCI₂(g) A reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.175 M at 1000 K. What is the equilibrium concentration of COCl2 at 1000 K? = 255 at 1000 K.
Please don't provide handwritten solution ..... Consider the equilibrium system involving the decomposition of methylene chloride. 2CH2Cl2(g) CH4(g) + CCl4(g) K = [CH4] [CCl4] = 8.62 at 361 K [CH2Cl2]2 A flask originally contains 0.349 M methylene chloride. Calculate the equilibrium concentrations of the three gases.
For the reaction 2HI (g)<----> H2 (g) + I2 (g) Kc=1.84. If a reaction mixture initially contains 1.00M HI, 2.00M H2 and 2.0M I2. Calculate the reaction quotient and the value of [HI] at equilibrium.
Bromine monochloride is synthesized using the reaction. Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 202.0 L flask initially contains 0.965 kg of Br2 and 1.032 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: 13.62 percent yield: Incorrect What is the percent yield of BrCl? 86 Incorrect 0.0 g %
The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) → H₂(g) + 12 (9) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. HI [H₂] [1₂] = = = M 3 M
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dont provide hnadwritng solution....
For items 10-12. The decomposition of NH4Cl (s) at a given temperature of 548 K, the Kp = 0.01072. NH4Cl (s) = NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4Cl (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NH4Cl (s) NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? A. 2.48 x 10-⁹ B. 2.35 x 10-4 C. 1.59 x 10-3 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H= 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K
4. Explain the effect of each of the following errors on the value of Ksp. Would you expect the Kp values will be higher than expected, lower than expected, or the same as expected, if: (a) A small amount of solid Ca(IO3)2 was present in the solution collected. (b) The graduated cylinder was not rinsed after transferring each sample into the flask or the rinses were not added to the respective sample.
For the reaction A + B --> 2 C, Kç = 0.16. A 2.00 L flask is filled with 1.00 mol A and 1.00 mol B, and allowed to come to equilibrium. Determine the concentrations, in moles/liter, of A, B and C at equilibrium. (Do not input units, 3 sig figs). A = B = C =