If 21.01 g of NO and 99.42 g of Br2 are placed in a 1.35-L reaction vessel and sealed and the mixture is heated to 300 K and chemical equilibrium is achieved and the concentration of the product nitrosyl bromide is 0.4128 M that what is the value of Ko to 2 decimal places? Кс 2NO (g) + Br2(8) H 2NOB (g)

At 460 °C, the reaction * NO(g) + SO3(g) SO2(g) + NO2(g) has Kc = 85.0. Suppose 0.109 mol of SO2, 0.0612 mol of NO2, 0.0755 mol of NO, and 0.118 mol SO3 are placed in a 10.0 L container at that temperature. What will the concentrations of all the gases be when the system reaches equilibrium? %3D [SO2) = M i [NO2] = M %3D [NO] = i M [SO3] = i M

Interconvert K, and Kc values. Calculate Kp for the following reactions at the indicated temperature. (a) PCl3(g) + Cl₂(g)=PCI5(g) Kc = 200 at 479 K Kp = (b) NH4l(s) NH3(g) + HI(g) K = 1.34×10-³ at 651 K Kp =

At 200 °C, Kc = 1.40 x 10-10 for the reaction N₂O(g) + NO₂(g) = 3NO(g) If 0.272 mol of N₂O and 0.523 mol NO2 are placed in a 4.00 L container, what would the NO concentration be if this equilibrium were established? [NO] = i M

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

Find the equilibrium concentration expression for the following reaction 4HNO3(aq)+3Ag(s)-->3AgNO3(aq)+NO(g)+2H2O

For the reaction   2H2O(g)↽−−⇀2H2(g)+O2(g)   the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.590 M, and [O2]=0.750 M. What is the equilibrium constant for this reaction? Kc=