+ Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH₁, 2.8 mol H2S, 0.63 mol CS2, and 0.042 mol H2 at 93.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH(g) + 2 HS(g) = CS₂(s) + 4 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. [0.042]4 Кс = [2.8]² [1.2] || 6.6 × 10-8 RESET [1.2] [2.8] [0.63] [0.042] [0.24] [0.56] [0.13] [0.0084] 2[2.8] [2.8]² 2[0.56] [0.56]² 4[0.042] [0.042]4 4[0.0084] [0.0084]* 0.063 16 6.6 × 10-8 1.5 × 107 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH, 2.8 mol H2S, 0.63 mol CS2, and 0.042 mol H2 at 93.0 °C. What are the values of Kc and Kp for the reaction at this temperature? Complete Parts 1-2 before submitting your answer. CH(g) +2 HS(g) = CS₂(s) + 4 H2(g) < PREV 1 2 Based on your value of Kc, determine the value of Kp under these conditions. Kp = 6.0 × 10-5 RESET 0.063 16 6.6 × 10-8 1.5 × 107 3.8 × 10-6 6.0 × 10-5 7.3 × 10-11 2.0 × 10-6 1.1 × 10-⁹

4) At high temperatures nitrogen (N₂) and oxygen (O₂) will react to form NO. N₂(g) + O₂(g) 2 NO(g) The value for the equilibrium constant for reaction 4.1 is Kc = 2.7 x 10-¹7 at some temperature T. A system initially has [N₂] = 0.0800 M and [0₂] = 0.0500 M. There is no NO initially present in the system. Find the value for [NO] that will be present at equilibrium. (4.1)

The equilibrium constant, Kc, for the following reaction is 2.0. If the equilibrium mixture contains 1.8 M NO and 0.70 M Br2, what is the molar concentration of NOBr? 2NOB1(g) = 2NO(g) +Br2 (g) Express your answer to two significant figures and include the appropriate units.

Initial (M) Change (M) Equilibrium (M) Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO₂(g) NEXT A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. -0.00875 0.0209 0 0.00875 2SO₂(g) Question 20 of 33 2.00 0.0216 0.0432 0.0148 0.0296 0.0041 O₂(g) 0.0175 2 0.0129 -0.0175 0.0061 RESET -0.0350 0.0257 2SO₂(g)