An equilibrium mixture has 0.583 mol of sulfur dioxide and 0.240 mol of bromine in a rigid 1.25 -L container. The equilibrium concentration of SO2Br2(g) is 0.670 M. What is the value of the equilibrium constant, Kc for this reaction? Report your answer to THREE significant figures. SO2(g) + Br2(g) ⇌ SO2Br2(g)

For the reaction 2CO2 (g)    ⇌       2CO (g) + O2 (g), Kc = 6.4 x 10-7.  If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

A chemist places 1.00 mol of each hydrogen and carbon dioxide in a 1.25-L container at 800oC. This reaction occurs:H2(g) + CO2(g) ⇌ H2O(g) + CO(g)When equilibrium is reached, 0.49 mol of gaseous carbon monoxide is in the container. Based on this information, what is the value of the equilibrium constant, K?

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.87 × 10⁻³ at a certain temperature. If 5.00 g of solid PH₃BCl₃ and 0.0700 g of BCl₃ are added to a 4.500 L reaction vessel, what will the equilibrium concentration of PH₃ be? PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g)   1.) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms   2.) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown.   3.) Based on your ICE table, set up the expression foe Kc in order to determine the unknown.   4.) Based on your ICE table and expression for Kc, solve for the partial pressure of PH3, at equilibrium.

Consider the following reaction between nitrogen and oxygen and its equilibrium constant at 2000 °C: N2(g) + O2(g) ⇌ 2 NO(g)Kc = 4.10 × 10−4 a)Is the formation of nitrogen monoxide favored at 2000 °C? Explain your answer without doing a calculation. b)What is the nitrogen monoxide concentration when a mixture of 0.40 mol of nitrogen gas and 0.30 mol of oxygen gas reaches equilibrium in a 2.0-L container at 2000°C?

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

Consider the following reaction and associated equilibrium constant at 430 K. 12 (g) + Br2 (g ) ⇌ 2 IBr (g) Kc = 278 If the reaction begins with 0.250 mol of IBr in a 2.00 L flask, calculate the concentration (mol/L) of IBr at equilibrium. Enter your answer with no units. Do not give handwriting solution.

Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBr has a value Kc equal to 3.07 × 10⁻⁴ at 297 K. If an initial solution of 0.20 M NOBr decomposes, what will the concentration of NO be at equilibrium?   2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

For the reaction 2CO2 (g) ⇌ 2CO (g) + O2 (g), Kc = 6.4 x 10-7. If 1.0 x 10-3 moles of CO2 is placed in a 1.0 liter vessel, what are the concentrations of all species at equilibrium?

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