For each of the following reactions, write the appropriate equilibrium equation. (Equilibrium expressions take the general form: Keq = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) (a) PCl5(g) equilibrium reaction arrow PCl3(g) + Cl2(g) (b) C(s) + H2O(g) equilibrium reaction arrow H2(g) + CO(g)
For each of the following reactions, write the appropriate equilibrium equation. (Equilibrium expressions take the general...
For each of the following
reactions, write the appropriate equilibrium equation. (Equilibrium
expressions take the general form: Keq =
[C]c / [A]a . [B]b. Subscripts and
superscripts that include letters must be enclosed in braces
{}.)
(b) H2(g) + F2(g) = 2 HF(9) chemPad Help x.x = Greek [H2][F2] KeqHF12 K_{eq} = [H_2][F_2/[HF)^2 Your answer contains a division sign (/) in an unexpected location.
Nitrogen and oxygen react at high temperatures. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) ΔH = 182.6 kJ (a) Write the expression for the equilibrium constant (Kc) for this reversible reaction. (Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.)
Write the dissociation reaction and the corresponding Ka equilibrium expression for each of the following acids in water. (For the dissociation reaction, include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients. Concentration equilibrium expressions take the general form: Kc = [C]c / [A]a . [B]b. Subscripts and superscripts that include letters must be enclosed in braces {}.) (a) HC7H13O2(aq) dissociation reaction: equilibrium expression: (b) Cr(H2O)63+ dissociation reaction: equilibrium expression: (c) C3H7NH3+ dissociation reaction: equilibrium expression:
1. Write the equilibrium constant expressions (Kc) for the following reactions: (a) CO (g) + H2O (g) ⮂ CO2 (g) + H2 (g) (b) CH4 (g) + 2H2S (g) ⭢ CS2 (g) + 4H2 (g) (c) COCl2 (g) ⮂ Cl2 (g) + CO (g) (d) 2HI (g) ⮂ H2 (g) + I2 (g) (e) PCl3 + Cl2 (g) ⮂ PCl5 (g) (f) 2H2 (g) + O2 (g) ⮂ ...
Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds. (For the ionic equations, include states-of-matter under the given conditions in your answer. Solubility equilibrium expressions take the general form: Ksp = [An+ ]a . [Bm− ]b. Subscripts and superscripts that include letters must be enclosed in braces {}. For example: Ksp=[A+]2.[B2-] must be typed using K_{sp}=[A^+]^2.[B^2-] (a) Ag2CrO4 Net ionic equation Solubility product expression (c) Sn(OH)2 Net ionic...
write the equilibrium constant expressions for each of the following chemical reactions. a utch 3. Write the equilibrin L reactants a) CH3OH (g) → CO (g) + 2H2 (g) b) C3H8 (g) + 502 (g) 3CO2 (g) + 4H2O(g) c) N2(g) + O2(g) + 2NO(g) 4. For each of the following values of K, indicate whether the forward reaction, reverse real or neither would be favored. a. Keq = 3.7 x 108 (K>>>1) b. Keq = 4.1 x 10-3(K«<<l) c....
Each of the following equilibrium constant expressions has a mistake. Identify the mistake and pick the correct expression for each of the following reactions at equilibrium. (a) 4 NH3(g) + 6 NO(g) equilibrium reaction arrow 7 N2(g) + 6 H2O(g) Kc = [NH3]4[NO]6 [N2]7[H2O]6 error in the equilibrium expression: (Select all that apply.) Some products or reactants are missing. Some products or reactants are incorrectly included. The products and reactants have been switched. Superscripts are missing. Superscripts are incorrectly included....
(A) Does the equilibrium mixture contain products, reactants, both or none? (A1) 2O3(g) ⇌ 3O2(g) K = 5.9 x 1012 (A2) H2(g) + I2(g) ⇌ 2HI(g) K = 54 (C) Write the expression for Kc (C Part 1) PCl3(l) +Cl2(g) ⇌ PCl5(s) (a) Kc = [PCl5]/([PCl3] [Cl2]) (b) Kc = ([PCl3] [Cl2])/[PCl5] (c) Kc = 1/([PCl3] [Cl2]) (d) Kc = 1/[Cl2] (C Part 2) Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g) (a) Kc = ([Fe]3[H2O]4)/( [Fe3O4] [H2]4) (b) Kc =...
The equilibrium constant for the following reaction is 1.42×10-3 at 179 °C. PCl5(g)<-->PCl3(g) + Cl2(g) K = 1.42×10-3 at 179 °C Calculate the equilibrium constant for the following reactions at 179 °C. (a) PCl3(g) + Cl2(g)<--> PCl5(g) K = (b) 2 PCl5(g)<-->2 PCl3(g) + 2 Cl2(g) K =
Write the expressions for the equilibrium constants of the following reactions, that includes the mass action relationships (i.e., the ratio of standardized partial pressures) and the value of the equilibrium constant calculated from the Gibbs energies of reaction: a) CO2(g)+Cl2(g) <->COCl(g)+Cl(g) b)2SO2(g)+)O2(g) <-> 2SO3(g) c)H2(g)+Br2(g) <-> 2HBr(g) d)2O3(g) <-> 3O2(g)