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![Express the equilibrium constant for the following reaction.
7 H 2(8) + 7 Br 2( g) = 14 HBr( g)
[H2] [Br2]
K =
[HBr?
[HBr]14
K =
H2B2
[H2][Br2]
K =
[HBr]
[HBr]
K =
[H2 Br27
[HBr]14
K =
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- In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)Express the equilibrium constant for this reaction: N2(g) + 3 H2(g) <=> 2 NH3(g) K = [NH3]2 / ([NH3]2 x [N2]) K = ([NH3]2 x [N2]) / [H2]3 K = ([N2] x [H2]3) / [NH3]2Write the equilibrium constant expression (Kc) for the reaction below 2P2O5(g) + 10Cl2(g) ⇌ 4PCl5(aq) + 5O2(g)
- What is the equilibrium constant for 2 C2H4(g) + 2 H2O(g) ⇌ 2 C2H6(g) + O2(g), Is it Heterogenous or Homogenous?If the equilibrium constants for the two reactions 2 HCl(g) H2(g) + Cl2(g) K1 = 4.36x10-2 and I2(g) + Cl2(g) 2 ICl(g) K2 = 8.92x10-6 are denoted K1 and K2 respectively, then the equilibrium constant, K3, for the reaction below is 2 HCl(g) + I2(g) 2 ICl(g) + H2(g) K3= ?Consider the mixing of 25.00 mL of 0.0500 M Pb(NO3)2 with 25.00 mL of 0.0500 M NaCl and the equilibrium reaction, PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq) Ksp = 1.20 x 10-5 What is the molar concentration of Pb2+ in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the molar concentration of Cl- in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the ion product (Q)? Will a precipitate form? (yes or no)
- Write the reaction quotient, Qc, and the equilibrium constant, Kc, for 2C3H8(g) + 10O2(g) ⥫⥬ 6CO2(g) + 8H2O(g)Express the equilibrium constant for the following reaction: 2 CH2Cl2 (g) + Cl2 (g) ⇌2 CHCl3 + H2 (g) k=?Write the equilibrium constant for the reaction CH4(g) + 3 Cl2(g) ⇋ CHCl3(l) + 3 HCl(g), with the gases treated as perfect.
- At 500 K, the equilibrium constant for this reaction: X2(g) + 2Y2(g) ⇌ 3Z2(g) is Kc = 0.222. At the same temperature, what would be the Kc for the following reaction: Z2(g) ⇌ 1/3X2(g) + 2/3Y2(g)?A. Determine the value of the equilibrium constant, Kgoal for the reaction CO2(g)⇌C(s)+O2(g)CO2(g)⇌C(s)+O2(g), Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g)2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = K1 = 5.40×10−165.40×10−16 2. 2H2(g)+O2(g)⇌2H2O(l)2H2(g)+O2(g)⇌2H2O(l), K2 = K2 = 1.06×10101.06×1010 3. CH3COOH(l)⇌2C(s)+2H2(g)+O2(g)CH3COOH(l)⇌2C(s)+2H2(g)+O2(g), K3 = K3 = 2.68×10−92.68×10−9 Express your answer numerically. B. Determine the equilibrium constant, Kgoal for the reaction 4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=?4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=? by making use of the following information: P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019 PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2 Express your answer numerically.The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in Molarity at equilibrium? 1.97 x 10-2 2.78 x 10-2 2.38 x 10-2 1.74 x 10-2 3.24 x 10-2 2.99 x 10-2 2.57 x 10-2 2.11 x 10-2 1.55 x 10-2 1.35 x 10-2
