(4) Assume that the change in concentration of N2O4 is small enough to be neglected in the following problem. (a) Calculate the equilibrium concentration of both species in 1.00 L of a solution prepared from 0.129 mol of N₂O4 with chloroform as the solvent. N₂04 (9) 2 NO₂ (g) Kc = 1.07 x 10-5 in chloroform (b) Show that the change is small enough to be neglected.

(4) Assume that the change in concentration of N2O4 is small enough to be neglected in the following problem. (a) Calculate the equilibrium concentration of both species in 1.00 L of a solution prepared from 0.129 mol of N₂O4 with chloroform as the solvent. N₂04 (9) 2 NO₂ (g) Kc = 1.07 x 10-5 in chloroform (b) Show that the change is small enough to be neglected.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 78QAP: When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white...

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When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)
(a) What does it mean when the reaction quotient, Q, is numerically equal to the equilibrium constant, Kc? (b) What does it mean when it is less than the equilibrium constant? (c) What does it mean when it is less than the equilibrium constant?
If the theoretical reaction is given by: 3A(g) + B(g) = 2Cg where K = 100, what is the equilibrium constant K for 4C(g) = 6A(g) + 2B(g)?
starting with 1.2 M A and 0.25 M B, the equilibrium concentrations of A is found to be 0.75. 2A=B. (a) what is the equilibrium constant for this reaction.(b) what is the effect of catalyst on the equilibrium concentration of A? (c) If you assume that the reaction is aqueous, how is the equilibrium affected by the addition of the solvent (what happns when you double the solvent but not the solutes?)
Write an expression for the equilibrium constant for this reaction: N2O4(g)+ O3(g)=N2O5(s)+O2(g)
The thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1
Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400° C established the concentration of N, to be 1.2 M and the concentration of H, to be 0.24 M. N,(g) +3H,(g) =2NH;(g)K¸=0.50 at 400° C. What is the equilibrium molar concentration of NH, 13? A 0.091 B 0.0091 0.0083 0.24
The hydrogenation of pyridine to piperidine C;H;N(g) + 3 H2(g) 2 C;H,N(g) is an équilibrium pročess whose équilibrium constant is given by the equation 10.560 K log10 K = -20.281 + T (a) Calculate the value of K at T = 500 K. (b) If the partial pressure of hydrogen is 1.00 atm, what fraction of the nitrogen is in the form of pyridine mol- ecules at T = 500 K?
(a) If the molar solubility of YF, at 25 °C is 4.23e-06 mol/L, what is the Kep at this temperature? Ksp (b) It is found that 5.73e-05 g of Znj(AsO4)2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility product constant for Zn (ASO4)2- Kap- (c) The Kap of ZnCO, at 25 °C is 1.46e-10. What is the molar solubility of ZnCO₂? solubility mol/L
2:25 1 Question 17 of 25 Submit Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O, and 0.200 mol N20 and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N20(g) + 3 O2(g) =4 NO2(g) 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 N20(g) + 3 O2(g) = 4 NO2(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190 0.0410 0.0710 0.0360 0.180
Write the equilibrium constant for the reaction P4(s) + 6 H2(g) ⇋ 4 PH3(g), with the gases treated as perfect.