For the reversible reaction N2 (g) + O2 (g) the concentrations at equilibrium are [N2] = 0.36 Mand [O2] = 1.1 M, and K= 2.1 x 10-3. Find [NO] at equilibrium. = 2NO(g) M NO

Consider the following reaction: COCI2(g) + CO(g) + Cl2(g) A reaction mixture initially contains 1.6 M COCI2. Determine the equilibrium concentration of CO if Kc for the reaction at the temperature is 8.33 x 104. Calculate this based on the assumption that the answer is negligible compared to 1.6. + indicates an equilibrium arrow. 4.2 x 10-4 M 1.5 x 103 M 3.7 x 10-2 M 2.1 x 102 M 1.3 x 103 M

At 2000°C the equilibrium constant for the reaction is Kc = 2.4 x 10³. 2 NO(g) = N₂(g) + O₂(g) If the initial concentration of NO is 0.100 M, what are the equilibrium concentrations of NO, N₂, and O₂? [0₂] 0.049 [N₂] 0.049 [NO] 0.002 M M X M

Consider the following reversible reaction equation: 2502(g) + Oz(g) → 2503(g) Ka = 1.2 x 103 Complete the following sentences (a-e) by selecting the best choice from the dropdown menus. a) This is an example of a v equilibrium. b) At equilibrium, this system will contain mostly c) If more SO2 is added to this system at equilibrium, the reaction will shift towards the d) If oxygen gas is removed from this system at equilibrium, the reaction will shift towards the e) If the volume of this system at equilibrium is increased, the reaction will shift towards the

5. A container is filled with 0.450 M CH3OH (g) and 0.050 M H2(g). When equilibrium is established at some unspecified temperature, [CH3OH] -0.200 M. Complete the following I-CE table and determine the equilibrium constant (Kc) of this reaction. Initial concentration / M Change in concentration/M Equilibrium concentration / M CO (g) 0.000 + 2 H2(g) 14 CH₂OH (g) 0.050 0.450

1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).

For the reversible reaction N2​(g)+O2​(g)2NO(g) the concentrations at equilibrium are [N2] = 0.76  M and [O2] = 0.22  M, and K = 2.1 × 10–3. - Find [NO] at equilibrium

Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]=  M.  Round your answer to 3 significant figures. c) [H2] =  M. Round your answer to 2 significant figures. d) [CO]=  M. Round your answer to 2 significant figures. e) [H2O]=  M.  Round your answer to 2 significatnt figures

NA van wwwwwwww 1. For the reaction, 2 NO (g) + 2 H₂ (g) = following equilibrium concentrations: [NO]= 8.1 x 10-³ M [N2] = 0.053 M N₂ (g) + 2 H₂O (g), calculate Keq given the [H₂] = 4.1 x 10-5 M [H₂O]= 2.9 x 10-³ M 2. Given the reaction, UO2 (g) + 4 HF (g) = UF4 (g) + 2 H₂O (g), predict the effect each of the following will have on the equilibrium of the reaction (shift to the reactant side, the product side, or no shift). a. Uranium dioxide (UO2) is added. c. Water vapor is removed. b. Hydrogen fluoride (HF) reacts with the walls of the reaction vessel. - 3. At a certain temperature, Keq = 150 for the reaction being studied in today's lab. Use Equation (3) to calculate the concentrations of Fe³+ and SCN in a solution that has an equilibrium FeSCN2+ concentration of 4.5 x 105 M. Assume the equilibrium concentrations of Fe³+ and SCN are equal.