2. Consider the following reaction: COCl2(g) <--> CO(g) + Cl₂(g) A reaction mixture initially contains 1.6 M COCI2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. A) 3.7 × 10-2 M B) 1.5 × 10-3 M C) 4.2 × 10-4 M D) 2.1 × 10-2 M -3

Consider the following chemical equilibrium: N₂ (g) + 3H₂(g) 2NH3(g) с Now write an equation below that shows how to calculate K from K for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator. K₁ = 0 P 00 X 5 010

The equilibrium constant, K, for the following reaction is 1.0 x 10 -5 at 1500 K. N2(g) + O2(g) <---> 2 NO(g) If 0.750 M N2 and 0.750 M O2 are allowed to reach equilibrium at 1500 K, what is the concentration of NO?   a. 2.4 x 10-3M   b. 6.7 x 10-4M   c. 5.5 x 10-3M   d. 2.7 x 10-3M   e. 1.2 x 10-3M

Question 13 of 50 Consider the equilibrium system described by the chemical reaction below. When 1.50 mol of CO, and an 10.0 mol solid carbon are heated in a 20.0 L container at 1100 K, the equilibrium concentration of CO is 0.0700 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for 2 this reaction. C(s) + CO,(g) =2 CO(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C(s) CO,(9) 2 СО(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 1.50 10.0 20.0 0.500 0.150 0.0750 0.0700 -0.0700 0.140 -0.140 0.0350 -0.0350 0.110 0.0400 0.0050 1L

Consider the following reaction: COCl2(g)  ⇌   CO(g) + Cl2(g)  A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is 8.33 ×  10 -4 . Calculate this based on the assumption that the answer is negligible compared to 1.6.   A 1.3 × 10-3 M   B 1.5 × 10-3 M   C 2.1 × 10-2 M   D 3.7 × 10-2 M   E 4.2 × 10-4 M

An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =

CO(g) + H₂O(g) ⇒ H₂(g) + CO₂(g) K = 7.3@823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H2O. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M

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