[0] Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 x 10³ at a certain temperature. If the equilibrium concentrations of H₂ and F₂ are both 0.0021 M, determine the concentration of HF at equilibrium. H₂(g) + F₂ (g) = 2 HF(g) Kc = [0.0021] 2[0.0021] 2[0.0011] [0.0011]' Question 17 of 19 1 If [x] represents the equilibrium concentration of HF, 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. R 2 [2x] NEXT> = 2.1 x 10³ [x]² [2x]¹ Submit RESET [0.0011]

Suppose a 250. mL flask is filled with 1.7 mol of NO2, 0.80 mol of CO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g) + CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 2.90 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g)  ->  2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!)   b. If the container size is 3.0 L, what is the value of the equilibrium constant?

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1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).

2 A reaction quotient, Q, is calculated to be 3.2 x 10. The equilibrium constant for the same reaction is 5.4 x 10³. Which statement is correct? a The system is at equilibrium. b The concentrations of the products are greater than their concentrations at equilibrium. The system will attain equilibrium by moving to the right. The system will attain equilibrium by moving to the left. More information is needed to determine which statement is correct. C d e

When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)

For the reaction 2NO(g) + O2(g) → 2NO2(g) at a certain temperature, the equilibrium concentrations were found to be [NO2] = 5.7 × 10–3 M, [O2]= 1.0 × 10–2 M, and [NO] = 2.0 × 10–3 M. Calculate the value of the equilibrium constant from these data.