Practice ProblemATTEMPT
For each reaction, predict the direction of shift caused by increasing the volume of the reaction vessel.
(a)
(b)
(c)
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Chemistry
- 5. Ka of HF is 6.80 × 104, what is the value of the equilibrium constant of the following reaction at 25 °C? F (aq) + H₂O(1) HF(aq) + OH(aq) (A) 6.80 x 104 -11 (B) 1.47 x 107 (C) 1.00 x 10-14 (D) 6.80 x 10-13arrow_forward4 (a) Calculate the value of Kc for the reaction: PC15 ( PC13 ( + Cl2 (g) AH = Positive Given that when 8.4 mol of PC15 (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PC15 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (i) Increasing temperature (ii) Lowering the concentration of chlorine (Cl₂) (iii) Addition of a catalystarrow_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
- The equilibrium constant (KC) is 10.0 x 10-10 at 800 K for the reaction. N2O3 (g) ⇄ NO2 (g) + NO (g) (2a)Write the equilibrium expression for this reaction. (2b) What is the value of KP at this temperature?(2c) What is the value of KC for the reverse reaction?arrow_forwardCalculate the value of K of MX using the following reaction. sp M* (aq)+X" (aq)→MX(s) log K = 8.16 (A) 1.44 x10 (В) 6.9х10-5 (C) 6.9×10-9 (D) 1.44×10arrow_forwardWhich of the following statements is (are) true? (Select all that apply.) If equilibrium constants for the chemical reaction N2(g) + O2(g) : = 2 NO(g) are K, = 1.1 x 103 and 3.6 x 103 at 2,200 K and 2,500 K, respectively, then the reaction is exothermic. If Q < K then the reactant concentrations will be decrease as the reaction proceeds to equilibrium. Concentration of the products equals the concentrations of the reactants. If the reaction, C(s) + 2H2(g) = CH4(g) is at equilibrium, adding solid carbon will cause the reaction to shift in the forward direction. None of these statements are true. O At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.arrow_forward
- 5.Write equilibrium expressions for each of the following reactions: (a) CaCO3(s) →*CaO(s) + CO,(g) (b) Hg() + Hg²+ (aq) → Hg2+ (aq) (c) 2Fe(s) + 3H₂O(1) (d) O₂(g) + 2H₂(g) ● ● ● Fe₂O3(s) + 2H₂(g) -2H₂O(1).arrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forwardCalculate ΔG° (answer in kJ/mol) for each of the following reactions from the equilibrium constant at the temperature given. (e)CH3NH2(aq)+H2O(l)⟶CH3NH3+(aq)+OH−(aq) T=25°C Kp=4.4×10−4 (f)PbI2(s)⟶Pb2+(aq)+2I−(aq) T=25°C Kp=8.7×10−9arrow_forward
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