Consider the reaction: P(s) + 3/2Cl₂ (g) ⇒ PCl3 (g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: P(s) + 5/2Cl₂ (g) ⇒PC15 (9) K₁ PC13 (g) + Cl₂ (9) ⇒ PC15 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K² if the first equilibrium constant should be squared. K =

Write the equilibrium law for the following reaction:

Consider the chemical reaction system represented by the following equation: 2 SO2 (g)  + O2 (g)  ⇆   2 SO3 (g)  The initial concentrations were 0.40 M SO2 (g) 1.6 M O2 (g) and 29.7 M 2 SO3 (g).  The equilibrium concentration of SO2 is 1.2 M.  Determine the value of Keq.

Write the equilibrium 6H2O(g) + 6CO2(g) C6H12O6(s) + 6O2(g)

At a certain temperature, Kc = 6.0 x 10^-4 for the reaction between sulfur trioxide gas and gaseous hydrogen fluoride to produce gaseous sulfur hexafluoride and water vapour: SO3(g) + 6HF(g) = SF6(g) + 3H20(g) Calculate the equilibrium concentration of sulfur hexafluoride that would result if 1.8 mol of sulfur trioxide was mixed with 5.6 mol of hydrogen fluoride in a 2.1 L container.

The equilibrium constant, Kc, is given for one of the reactions below. What is the value of the missing equilibrium constant, Ke? Cl₂(g) + H₂O(g) = 2 HCl(g) + O₂(g) K = 7.52 x 10-² 4 HCI(g) + O₂(g) = 2 Cl₂(g) + 2 H₂O(g) K = ? OK=177 K = 0.150 OK-5.66 x 10-3 OK 13.3 3 pts ) K = 3.65

4.

Consider the reaction: SO₂(g) + 1/2O₂(g) ⇒ SO3 (9) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K2, for the reactions below: 2S(s) + 30₂(g) ⇒ 2SO3 (9) K₁ S(s) + O₂(g) → SO₂(g) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K= An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.

Suppose a 500. mL flask is filled with 1.9 mol of Cl₂, 1.5 mol of CHC13 and 0.60 mol of HC1, The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g) The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. OM X

Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl,(g) = 2NOCI(g) is 2 x 10° at a certain temperature. In an experiment, 3.00 x 10-2 mole of NO, 4.70 × 103 mole of Cl,, and 6.60 moles of NOCI are mixed in a 1.30-L flask. What is Q. for the experiment? X 10 (Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the left. The reaction will proceed to the right. The reaction is at equilibrium.