Determine the values of Kc that correspond to the following values of Kp. 1.) SO2CI2(g)—›‹—SO2(g)+CI2(g) Kp=2.9×10^-2 at 303K 2.) 2 NO2(g)—›‹— 2 NO(g)+O2(g) Kp=0.275 at 700k 3.) CO(g)+CI2(g)—›‹—COCI2(g) Kp=22.5
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- 3) Based on the information below, determine the value of the unknown equilibrium constant, Kc. 4 CO2 (g) + 2 H2O (g) « 4 O2 (g) + 2 CH2CO (g)Kc = 3.7 x 1017 CO2 (g) + 2 H2O (g) « CH4 (g) + 2 O2 (g)Kc = 8.3 x 10-15 CH4 (g) + CO2 (g) « CH2CO (g) + H2O (g)Kc = ?Given C2HGO(g) + 302(g)=2CO2(g) + 3H20(g) Kp = 7.2 2C2H,O(g) + 502(g)= 4CO2(g) + 4H2O(g) Kp = 7.1 x 101 calculate K, for 2C2H6O(g) + O2(g)= 2C2H40(g) + 2H20(g) Report your answer with two significant figures. Do NOT include units in your answer.2) Based on the information below, determine the value of the unknown equilibrium constant, Kc. 2 NOCl (g) « 2 NO (g) + Cl2 (g)Kc = 2.4 x 10-7 1/3 Cl2 (g) + 2/3 NO (g) « 2/3 NOCl (g)Kc = ?
- Calculate Kc or Kp:CH4(g)+H2O(g)->CO(g)+3H2(g) Kp=7.7x10^24 (at 298 K)Calculate the value of the equilibrium constant, Kc, for the reaction Q(g) +X(g) 2M(g) + N(g) given that Kc = M(g)Z(g) Kcl = 3.14 6R(g) 2N(g) + 4Z(g) Kc2 = 0.561 3X(g) +3Q(g) 9R(g) Kc3 = 11.9› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6
- Calculate the value of the equilibrium constant, Kc, for the reaction Q(g) + X(g) 2 M(g) + N(g) given that Kc = M(g) = Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9 R(g) Kel : 3.49 Kc2 = 0.469 Kc3 = 14.4Consider the following reactions: CO (g) + 2 H2S (g) D CS2 (g) + H2O (g) + H2 (g) K1 = 1.3 x 105 ½ CH4 (g) + H2S (g) D ½ CS2 (g) + 2 H2 (g) K2 = 180 1. Find the equilibrium constant for: 2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g) 2. What molecules in the steps are reaction intermediates? 3. If 0.500 atm of CO, H2, CH4, and H2O are initially placed in the same container, then given your answer in part a., determine which direction the reaction will shift in order to establish equilibrium.Given the following reactions and the equilibrium constants CO (g) + H,0 (g) Co, (g) + H2 (g) K1 = 1.0 X 105 co (g) + 2 H2 (g) CH;OH (g) K2 = 1.4 X 107 Predict the equilibrium constant for Co, (g) + 3 H, (g) CH;OH (g) + H,0 (g) K = ? 4 O 13900000 O 140 O 0.00714
- Given these reactions and their equilibrium constants, CO(g) + 3 H₂(g) → CH4(g) + H₂O(g) K = 3.93 N₂(g) + H₂(g) = NH3(g) Kc = 0.324 determine Ke for the following reaction. CO(g) + 2 NH3(g) CH4(g) + H₂O(g) + N₂(g) Your Answer: Kc = 37.4a Suppose the reaction system CH4 (9) + 202 (g) = CO2(g) + 2H2O(1) has already reached equilibrium. The position of the equilibrium was shifted by removing any liquid water from the system. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. It will shift to the left. O It will not be affected.Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc1 = 2.3 × 10 – 7 2NO3(g) ⟷ 2NO2(g) + O2(g) Kc2 = 1.4 ×10 – 3 Calculate the equilibrium constant for the reaction: SO2(g) + NO3(g) ⟷ SO3(g) + NO2(g) A 1.3 × 10 – 2 B 1.6 × 10 – 4 C 78 D 6.1 × 103