Consider the following equilibrium reaction: A+ 2HF +CO {}2F_ _+ H_O, +CO2) (aq) (a) Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: i) ii) Action Add HF to the reaction Add Na₂CO3 to the reaction Add NaCl Add KF to the reaction Add CO₂ to the reaction Remove CO₂ from the reaction Remove HF from the reaction 3 (op) Increase pressure by reducing volume Cool the reaction mixture Heat the reaction mixture iii) Provide four suggestions to increase the amount of CO₂ gas generated. Shift Left Shift Right

Consider the following equilibrium reaction: A+ 2HF +CO {}2F_ _+ H_O, +CO2) (aq) (a) Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: i) ii) Action Add HF to the reaction Add Na₂CO3 to the reaction Add NaCl Add KF to the reaction Add CO₂ to the reaction Remove CO₂ from the reaction Remove HF from the reaction 3 (op) Increase pressure by reducing volume Cool the reaction mixture Heat the reaction mixture iii) Provide four suggestions to increase the amount of CO₂ gas generated. Shift Left Shift Right

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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Kc = 0.0600 at 500 °C. (a) Determine whether a mixture that contains 1.35 M N, 1.80 M H,, and 0.215 M NHa is at equilibrium? (b) If not, predict the direction in which a net reaction would occur to reach equilibrium? (c) How would each concentration of N2, H2 and NH3 change (increase or decrease) when the reaction reaches equilibrium?
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Consider the equilibrium below:If 2.4 mol of HCl was placed in a 0.8 L container and allowed to reach equilibrium, what wouldthe equilibrium concentration be for HCl(g) if the Keq = 56? 2HCl(g) <=====> H2(g) + Cl2(g)
For the following equilibrium reaction, determine the NO₂ expression NO CI(g) NO(g) + Cl(g) for the concentration of ko
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3. Several reactions are listed below with their equilibrium constant values. Place an "X" in the appropriate box in the Table to indicate your prediction for the direction of the reaction to produce mostly products (proceed Right) or mostly reactants (proceed Left)? Why? Equilibrium Reaction and/or Condition (a) NH4*(aq) + H₂O(l) NH3 (aq) + H3O+ (aq) (b) Mb + O₂ MbO2 (c) If Q = 8.3 x 106 for (b) above (d) If Q=1500 for (b) above (e) If for (b) above the following initial conditions exist: [Mb], = 2.04 x 104; [0₂]o= 3.00 x 10° M; [MbO₂]0=2.50 x 104 M (f) H₂SO3(aq) H*(aq) + HSO3(aq) K = 5.6 x 10-10 K = 8.6 x 105 K = 8.6 x 105 K = 8.6 x 105 K = 8.6 x 105 K = 0.0120 R L Reason
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What effect will increasing the temperature have on the system at equilibrium? C3H8(g) + 5 O2(g) ⟷ 3 CO2(g) + 4 H2O(l) ΔHo = -2220 kJ The value of K will increase, and the reaction will shift toward the reactants. The value of K will increase, and the reaction will shift toward the products. The value of K will decrease, and the reaction will shift toward the products. The value of K will decrease, and the reaction will shift toward the reactants.
Consider the following system at equilibrium: Fe2 O3 (s) + 3H2 (g) = 2 Fe (s) +3H2O (g) ΔΗ -98.7 kJ | If the volume was increased, what changes would have to occur to reestablish equilibrium? The concentration of H2 would increase. The concentration of H2 would decrease. The concentration of H20 would decrease. The concentration of H20 would increase. No change