A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700 M, [B] = 0.950 M , and [C] = 0.500 M . The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.510 M and [C] = 0.690 M . Calculate the value of the equilibrium constant, K.. Express your answer numerically.

At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6.  Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M.  Your answer should have two significant figures.

Suppose a 500. mL flask is filled with 0.70 mol of CO, 1.7 mol of NO and 1.0 mol of CO,. The following reaction becomes possible: NO, (g) +CO(g)- NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.97 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM Continue MacBook Air

A student adds 0.600 mol of methane gas, CH4(g) into a 2.00 L container and the methane forms ethyne, C2H2(g) and hydrogen gas, H2(g). At equilibrium, the container was found to contain 0.045 mol/L C2H2.a) Calculate the initial concentration of CH4. Then complete an ICE Table to organize the initial, change and equilibrium concentrations for this equilibrium system. Show any calculations needed. 2CH4(g) ⇄ C2H2(g) + 3H2(g)b) Calculate the equilibrium constant, Keq, for this equilibrium. Show all work.c) What is the equilibrium concentration of H2(g) ?

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Suppose a 500. mL flask is filled with 0.10 mol of O, and 1.6 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) =2NO (g) The equilibrium constant K for this reaction is 0.679 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. | M

Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²

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