For the reaction M₂+N₂⇌2MN, scene A representsthe mixture at equilibrium, with M black and N orange. If eachmolecule represents 0.10 mol and the volume is 1.0 L, how manymoles of each substance will be present in scene B when thatmixture reaches equilibrium?

At equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.100 M and [NO] = 0.400 M. N, (g) + 0,(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established? [NO]final = M

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

hydrogen sulfide is a pungent, poisonous gas. At 1400 K, an equilibrium mixture was found to contain 0.013 mol/L of hydrogen, 0.18 mol/L of hydrogen sulfide and an undetermined amount of sulfur in the form of S2 gas. If the value of Kc is 2.40 x10^-4 at this temperature what concentration of S2 is present at equilibrium?

At equilibrium, the concentrations in this system were found to be [N,] = [O,] = 0.200 M and [NO] = 0.500 M. N2(g) + O2(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NO]inal M

The equilibrium constant (K.) is 0.0025 at 2127°C. If an equilibrium mixture at this temperature contains 0.028 mol N2 and 0.053 mol O2 per liter, what is the concentration of NO?