102 for the reaction given below. H2(g) + F2(g)  2 HF(g) (a) Calculate the concentrations of all species in the equilibrium mixture produced by adding 3.4 mol of H2 and 3.4 mol of F2 to a 1.0 L container. H2       M F2       M HF       M (b) What would the equilibrium concentration of HF be if 1.1 mol of HF were removed from the equilibrium mixture in Part (a)?   M

Hydrogen iodide decomposes according to the reaction 2HI(g) = H₂(g) + 1₂ (g) A sealed 1.50-L container initially holds 0.00623 mol of H₂, 0.00414 mol of 1₂, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H₂(g) is 0.00524 M. What are the equilibrium concentrations of HI (g) and I₂ (g)? Round each of your answers to 3 significant figures. Part 1 of 2 [HI] = M Part 2 of 2 [¹2]eq = M x10 x10 X x Ś S

For the reaction 3 O2(g)  2 O3(g) The equilibrium constant, K, has the value 1.12  10-54 at a particular temperature. (b) If the equilibrium mixture is analyzed and [O2(g)] is found to be 3.71  10-2 M, what is the concentration of O3(g) in the mixture?  M

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

Determine the concentration of all species at equilibrium for each of the following original mixtures. At 40C K= 1.7*10^-5 2NOCl(g) ——-(reversible)—— 2NO(g) + Cl2(g) a) 2moles of NOCl 2 moles of NO 1 mole or Cl2 in 1.0L flask b) 1M concentration of all three gases

If this reaction is taking place in a 1.0L container, and 1.5 mol of SO2 were added to the reaction, whatwill the new concentrations of all fours gases be when equilibrium is reestablished?

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.