Iodine and bromine react to give iodine monobromide, IBr. I2(g) + Br2(g) ---- 2IBr(g) What is the equilibrium composition of a mixture at 126°C that initially contained 1.10 x 10^-3 mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant Kc for this reaction at 126°C is 72.1. [I2] =  M [Br2] =  M [IBr] =  M

The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCI3(g) + Cl₂(g) PCI5(g) Calculate the equilibrium concentrations of reactant and products when 0.587 moles of PCI3 and 0.587 moles of Cl₂ are introduced into a 1.00 L vessel at 500 K. [PCI3] = [Cl₂] [PCI 5] = = M M M

A student ran the following reaction in the laboratory at 1101 K:2SO2(g) + O2(g)      2SO3(g)When she introduced 0.104 moles of SO2(g) and 0.101 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 7.28×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

SC At a certain temperature, the equilibrium constant K for the following reaction is 506.: Br₂(g) + OC1₂(g) BrOCI(g) + BrCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 0.62 mol of Br₂ and 0.62 mol of OCI₂. What can you say about the composition of the mixture in the vessel at equilibrium? ! 1 What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. BrOCI(g)+BrCl(g) Q A What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 Br₂(9)+20C1₂(9) P 2 BrOCI(g)+2BrCl(9) Explanation NO 2 W S Check *3 # E Br₂(9)+OCL₂(9) D D DS 4 C R F % LO 5 O There will be very little Br₂ and OCl₂. O There will be very little BrOCI and BrCl. ONeither of the above is true. K = 0 K = 0 T MacBook Pro 20 ^ 6 G Y C & 7 H 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C U 00 8 J X I ( 9 K 0 0 < F

The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 4.05 L container at 673 K contains 2.71 mol of NH4I(s) and 0.262 mol of NH3, the number of moles of HI present is  moles. --- The equilibrium constant, Kc, for the following reaction is 6.30 at 723K.2NH3(g) N2(g) + 3H2(g)If an equilibrium mixture of the three gases in a 12.1 L container at 723K contains 0.250 mol of NH3(g) and 0.208 mol of N2, the equilibrium concentration of H2 is  M.

11. At a certain temperature, the equilibrium constant K for the following reaction is 9.0 x 10-8: N₂(g) + O₂(g) 2 NO(g) L Use this information to complete the following table. Suppose a 22. L reaction vessel is filled with 1.1 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO(g) N₂(9) + O₂(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 3 N₂(9)+30₂(9) 6 NO(g) Explanation # acBook Pro Check O There will be very little N₂ and 0₂. O There will be very little NO. O Neither of the above is true.. K = 0 K = 0 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center → a x10 alo Accessibility Ar