Consider the following equilibrium reaction: Ba;(PO,)2 (s) 3 Ba2*(aq) + 2 PO,3(aq) Ко 3 3.4 х 103 2.00 moles of each reactant and product were placed in 5.00 L of water, mixed and allowed to reach equilibrium. a) Write the Qc expression (LMA) for this reaction. b) Calculate the value of Qc. (Show all work for full credit.) c) In which direction will this reaction proceed to establish equilibrium. Explain your answer. d) Once equilibrium is reached, it was found that the barium ions CHANGED by 0.455 mol. How many moles of each reactant and product are present at equilibrium? (BOX YOUR FINAL ANSWER.)

Consider the following equilibrium reaction: Ba;(PO,)2 (s) 3 Ba2*(aq) + 2 PO,3(aq) Ко 3 3.4 х 103 2.00 moles of each reactant and product were placed in 5.00 L of water, mixed and allowed to reach equilibrium. a) Write the Qc expression (LMA) for this reaction. b) Calculate the value of Qc. (Show all work for full credit.) c) In which direction will this reaction proceed to establish equilibrium. Explain your answer. d) Once equilibrium is reached, it was found that the barium ions CHANGED by 0.455 mol. How many moles of each reactant and product are present at equilibrium? (BOX YOUR FINAL 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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Given the following reactions: 20 2D K =7.13 × 104 D = 2A+ 2B K = 6.93 x 10-2 1st attempt Feedback See Periodic Table O See Hint Calculate the value of the equilibrium constant for the following reaction. A +B = C * 37.266
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2. Consider a closed vessel containing a mixture of ideal gases A and B that undergo the chemical reaction: A=bB, where b is an unknown stoichiometric coefficient. The equilibrium mole fraction xд is measured but xB is unknown. The equilibrium mole fraction xд increases when the temperature in the vessel is increased with the pressure held constant and Ꮖ Ꭺ decreases when the pressure in vessel is increased with the temperature held constant. Explain these observations in terms of inequalities involving the enthalpy of reaction AH and the stoichiometric coefficient b in Eq. (7).
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5. Using the following data, calculate the equilibrium constant at T=1500 K for the reaction На (g) +1/2 О2 (g) Н.О (g) H2 O2 H2O Do (kcal/mol) 103.2 118.0 219.3 2 2 2 Or (K) Ov (K) 40.1, 20.9, 13.4 5360, 5160, 2290 85.3 2.07 6215 2256
The reaction P4(g) 2 2 P2(g) is endothermic and begins to occur at moderate temperatures. (a) In which direction do you expect deviations to occur from Boyle's law, P ∞ 1/V (constant T), for gaseous P4? (b) In which direction do you expect deviations to occur from Charles's law, V « T (constant P), for gaseous P4?
For the above reaction, if the value of Kp (expressed in terms of the partial pressures in atm) was 16.6 at 857°C, what would be the value of Keg (expressed in terms of the molar concentrations) at 857°C? (No units required.)
What is the mass-action expression, Qc, for the following chemical reaction? 4H30*(aq) + 2CI"(aq) + MnO2(s) Mn2+(aq) + 6H2O() + Cl2(g) ABBREVIATIONS AND SYMBOLS RFaraday constant A free energy atm frequency ugas constant NA gram "Chour e joule C kelvin dkilo prefix E liter Emeasure of pressure mm Hg vapor pressure Hmilli prefix S molal Kmolar CONSTANTS amount of substance ampere atmosphere atomic mass unit Avogadro constant Celsius temperature centi- prefix coulomb density electromotive force energy of activation enthalpy F molar mass mole Planck's constant M mol R-8.314 J motK R-0.08314 L bar mol K pressure rate constant reaction quotient second K speed of light k temperature, K time F-96,500 C mol F=96,500 J V'mol NA-6.022 x 102 mol h-6.626 x 10 MJS e-2.998 x 10 ms VP 0°C-273.15 K volt V I atm -1.013 bar - 760 mm Hg Specific heat capacity of H;0- 4.184 Jg'K m - volume M entropy equilibrium constant 1 PERIODIC TABLE OF THE ELEMENTS 18 1A 1 H 8A 2 13 14 4A 15 16 17 Не 1.008 ЗА 4.003 7A…
The KspKsp of a salt corresponds to a reaction with the following general format: salt(s)⇌mcation(aq)+nanion(aq)where mm and nn are the coefficients that balance the equation. Equilibrium constants follow the general format of products over reactants (excluding pure liquids and solids) with each species raised to the power of its coefficient in the balanced equation. KspKsp is no exception, so Ksp=[cation]m[anion]nKsp=[cation]m[anion]n Part A If 500.0 mLmL of 0.10 mol L−1 Ca2+mol L−1 Ca2+ is mixed with 500.0 mLmL of 0.10 mol L−1 SO42−mol L−1 SO42−, what mass of calcium sulfate will precipitate? KspKsp for CaSO4CaSO4 is 2.40× 10−52.40×10−5. Express your answer to three significant figures and include the appropriate units
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J R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H"(aq) + 4 e 2 H20 (1) 1.229 |Z2 (s) + 2 e → 2Z° (aq) 0.426 3+ (aq) + 3 е A' → A (s) 0.292 2 H20 (I) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 G2+ (aq) + 2 e G (s) - 1.245 (aq) + 2 e¯ → M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 MMZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 11 The electrode connected to the red wire (negative terminal on the battery) will... o produce bubbles and the pH will increase. o produce M (s) on the electrode and the pH will not change. o produce bubbles and the pH will decrease. o produce M (s) on the electrode and the pH will decrease. Question 12 The electrode…