What is the equilibrium constant expression for the reaction shown below? CACO3(s) R Ca²+ (s)ɛ + CO,²- (be) (be) O Keg = [Ca²+] / [ Co,²-] %D bə O Keg = [Ca2+][ Co,²-] OKea = 1/ [CaCO3] O Kea = [Ca²*][ CO3²-] / [CaCO3] OKea = 1/ [Ca²*][ CO3²-] bə

What is the value for Kc for the following reaction:  PbCl2(s) ⇌ Pb2+(aq) + 2 Cl-(aq), if PbCl2(s) = 1.50 grams, [Pb2+] = 1.6 × 10-2 M and [Cl-] = 3.2 × 10-2 M at equilibrium? 1.3 × 106 6.2 × 104 7.6 × 10-7 1.6 × 10-5

The following reaction in aqueous solution has Kc = 1 × 10-85 at a temperature of 25 °C. 7103(aq) + 9H₂0 + 7H*(aq) 1₂(aq) +5H5106(aq) What is the equilibrium law for this reaction? Ke = Ke Ke = Ke = [Hs 106]5 [103] [H+ ] [Hs 106]³[ 1₂ ] [103] [H+ ] [H5 106]³[ 12 ] [103] [H+ ][ H₂ O] [Hs 106]³ [103]

Write the balanced chemical equation corresponding to this expression for equilibrium constant expression.

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please help with this question. it's not an assay, but calculation. thanks

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328 K, the K eq for the reaction 2NO 2 (g) rightleftharpoons N 8 O 4 (g) is 1.5. Calculate the concentration of N_{2}*O_{4} present in equilibrium when [N*O_{2}] = 0.50 .

#9 part E

23. What is the correct form of the equilibrium constant Kc for the reverse reaction: N₂(g) + 3 H₂(g) = 2 NH3(g)? (A) Kc = [N₂][H₂]³ (B) Kc (C) Kc (D) Kc = (E) Kc = = 3 = 2[NH3] [N₂] + 3[H₂] [N₂] + 3[H₂] 2[NH3] 2 [NH3]² [N₂][H₂]³ 3 [N₂] [H₂]³ [NH3]²