Practice ProblemATTEMPT
For each change indicated, determine whether the equilibrium:
will shift to the right, shift to the left, or neither: (a) addition of
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Chemistry
- Consider 4 NH3(g)+ 5 O2(g)⇋4 NO(g)+ 6 H2O(g)(ΔH = -904.4 kJ). How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change. (a)Increase [H2O] (b)Decrease [O2] (c)Decrease the volume of the container in which the reaction occurs .(d)Add a catalyst. (e)Increase temperaturearrow_forwardSelect all that apply. For the following equilibrium system, which of the following changes will form more CaCO3? CO2(g) + Ca(OH)2(s) = CaCO3(s) + H2O(l) 0 ΔΗ =-113 kJ rxn Decrease temperature at constant pressure (no phase change). Increase volume at constant temperature. Increase partial pressure of CO2. Remove one-half of the initial CaCO3.arrow_forwarde) none of the above 25. If K = 0.124 for A2 + 2B = 2AB, what is the value of K, for the reaction 4AB 2A2 + 4B? a) 0.124 b) 0.248 c) 65.0 d) – 0.124 e) 4.03 f) none of the abovearrow_forward
- Question 2 Consider the following reactions, with equilibrium contants as shown: (1) C(s) + 0,(g) co,(g), K, (2) 2Ca(s) + O,(g)=2CaO(s). K, (3) 2Ca(s) + 2C(s) + 30,(g) =2CaCO,(s), K, In terms of K1, K2 and K3 , the equilibrium constant for the reaction CaO (s) +CO,(g) CACO,(s) can be expressed as: O a. O b. (K,) 2 + (K, + (K c. Od. O e. ) ( f. + (K None of the above.arrow_forwardCheck Your Understanding In each of the following, determine the direction in which the equilibrium will shift in response to the indicated stress. (a) N2 (g) + 3 H2 (g) 2 2 NH3 (g); pressure is decreased Answer + Shift toward reactants (b) CO2(g)+ H2 (g) 2 CO(g) +H2O(g); pressure is increased Answer no changearrow_forwardPractice Exercise At 1280°C the equilibrium constant (K.) for the reaction Br2(g) = 2Br(g) is 1.1 x 10-3. If the initial concentrations are [Br2] 6.3 x 10-2 M and [Br] = 1.2 × 10-2 M, calculate the concentrations of these species at equilibrium.arrow_forward
- For the equilibrium system N2044) # 2NO26) what is the equilibrium constant when [N2O4) is 1.5 x 10-3 M and [NO2] is 0.57 M? (B) 2.2 × 102 . (A) 3.8 × 10² (C) 4.6 × 10-3 (D) 2.6 × 10-3arrow_forwardPractice Exercise At 1280°C the equilibrium constant (K) for the reaction Br2(g) 2Br(g) is 1.1 x 10 . If the initial concentrations are [Br2] 102 M, calculate the concentrations of these species at equilibrium. 6.3 x 10 2 M and [Br] = 1.2 X !!arrow_forwardWhich of the following statements is true regarding chemical equilibrium? Question 4 options: A) When equilibrium has been reached, all chemical reactions have ceased. B) When equilibrium has been reached, the rates of the forward and reverse reactions are equal. C) When equilibrium has been reached, the rate constants of the forward and reverse reactions are equal. D) When equilibrium has been reached, the value of the equlibrium constant is 1. E) When equilibrium has been reached, the limiting reagent has been consumed.arrow_forward
- Incorrect Question 18 If 0.64 mol PCI, is placed in a 1.0 L flask and allowed to reach equilibrium at a given temperature, what is the final concentration of Cl₂ in the flask PCI5(g) --> PCl3(aq) + Cl2(g) Ke= 0.47 0.31 M 0.55 M 0.20 M 0.36 M C 0.96 Marrow_forwardQUESTION 18 Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204 (g) 2NO2 (g) A 1.000-L flask is filled with 0.73 mol of N204. At equilibrium, 0.31 mol of N2O4 remains. Determine the equilibrium constant K for this reaction. Express your answer in decimal notation to 2 decimal places.arrow_forwardA(g) ⇄ 2B(g)Initially, we have 1.583 mol/L of A.What is the concentration of A at equilibrium if the equilibrium constant Kc is equal to 30.9Give an answer with 4 significant figures.Suggestion: Do not round your answer too much and take the quadratic formula.arrow_forward
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