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
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- Nitrogen monoxide, NO, reacts with bromine, Br2, to give nitrosyl bromide, NOBr. 2??(?) + ??2(?) ⇄ 2????(?) A sample of 0.425 mole NO with 0.626 mole Br2 in a 1.25 L reaction vessel gives an equilibrium mixture containing 0.113 mol NOBr. What is the composition of the equilibrium mixture in term of Molarity?arrow_forwardWhat is the equilibrium constant of the following reaction at 25˚C? F⁻(aq) + H⁺(aq) ⇄ HF(aq) 1) 1.0 × 10⁻⁷ 2) 6.3 × 10⁻⁴ 3) 6.3 × 10¹⁰ 4) 1.6 × 10³ 5) 1.6 × 10⁻¹¹ Pls give typed answer no hand written .arrow_forwardA(g) ⇄ 2B(g)Initially, we have 0.914 mol/L of A.What is the concentration of A at equilibrium if the equilibrium constant Kc is equal to 34.7?Give an answer with 4 significant figures.Suggestion: Do not round your answer too much and take the quadratic formula.arrow_forward
- At a certain temperature, the value of the equilibrium constant, K, for the reaction represented below is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature? H2(g) + Br2(g) = 2HBr(g) (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5arrow_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_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_forward
- Which of the following is the correct equilibrium constant expression for the following reaction? A(s) ↔ B(g) + C(g)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_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
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