Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. Be sure to include the proper phases for all species within the reaction. AgNO3(s) →
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- Predict the net direction and whether Kc is greater or less than 1 for each of the following reactions (assume equal initial concentrations of all species):Use the reactions below and their equilibrium constants to predict theequilibrium constant for the reaction 2A(s)⇌3D(g).A(s) ⇌ 12 B(g)+C(g), K1=0.03343D(g) ⇌ B(g)+2C(g), K2=2.35Express your answer to three significant figures.The pH change during a reaction will be followed by inserting a pH probe into a relatively small volume of liquid sample, At least 1.5 cm of the pH probe must be immersed in the reaction solution. What is the best choice of reaction vessel for this reaction? a volumetric flask a Berzelius beaker a Griffin beaker a round bottomed flask an Erlenmeyer flask
- Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2.N2O4 (g) ⇌ 2 NO2 (g) (a) The equilibrium constant Kc at 25°C is 0,125. What percentage of dinitrogen tetroxideis dissociated when 0,0300 mol N2O4 is placed in a 1,00 dm3 flask and left to reachequilibrium?Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble.(a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO3(s) ⇌ Ca2+(aq) + CO32−(aq).Is Kc> 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba2+(aq) + 2PO43−(aq) ⇌ Ba3⎛⎝PO4⎞⎠2(s).Is Kc> 1, < 1, or ≈ 1? Explain your answer
- Answer the following questions regarding reactions involving ions in aqueous solution. i. Consider the following reaction, [A] + [B] ⇋ [TS]* → P , Write the equilibrium constant for the reaction above. ii. Prove that the following equation describes the rate of product formation for the reaction above.The reaction quotient, Q, is 9.00 × 10⁻¹² The Ksp of zinc fluoride is 3.04 x10⁻² at 25°C. Comparing this value to the Q obtained in the previous step, predict if the zinc fluoride will precipitate.The value of Kc for the reaction below is 0.210 at 373 K.N2O4 (g) ⇌ 2 NO2 (g)a. Mathematically determine in which direction the reaction will proceed if the reaction vesselinitially contains 0.300 M N2O4 at the given temperature?
- The equilibrium constant for the reaction below is K=5.87×105 at 277.0ºC.3 NO (g) ⇄ N₂O (g) + NO₂ (g) ΔHº = -155.52 kJUse the van't Hoff equation to calculate the value of the equilibrium constant for the reaction at 200.0ºC.Which of the following statements is TRUE? a. dynamic equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction b. the equilibrium constant for the forward reaction is equa to the equiloibrum constant for reverse reaction. c. A reation quotient Q larger than equilibrium constant K means the reaction will favor the production of more poroducts. d. dynamic equilibrium indicates taht the amount of reactants and products are equal. e. All of these are true which is correct?1. You determined the equilbrium constant, K eq^ prime for the reaction using a number of different [Fe^ 3+ ] 0; [SCN] 0 ratios . Does K eq depend on the relative intial concentraion of the reactants? Is this what you would expect? Explain your answer.