The equilibrium constant, Kc, for the following reaction is 0.00650 at 298 K. 2NOBr(g) 2NO(g) + Br₂ (9) If an equilibrium mixture of the three gases in a 15.6 L container at 298 K contains 0.201 mol of NOBr(g) and 0.284 mol of NO, the equilibrium concentration of Br₂ is M.

[Review Topics] [References] Use the References to access important values if needed for this question. 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 6.73 L container at 673 K contains 1.48 mol of NH4I(s) and 0.467 mol of NH3, the number of moles of HI present is mol. Submit Answer Q F4 % 5 Show Hint F5 ^ 6 Y Retry Entire Group 8 more group attempts remaining C F6 & 7 F7 * 8 F8 ( 9 F9 O ) O F10 P F11 Previous + F12 Next> delete

Suppose a 250. mL flask is filled with 0.90 mol of Cl₂, 1.2 mol of HCl and 2.0 mol of CC14. The following reaction becomes possible: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) The equilibrium constant K for this reaction is 0.702 at the temperature of the flask. Calculate the equilibrium molarity of CHC13. Round your answer to two decimal places.

The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 5.09 L container at 548 K contains 3.65 mol of NH4Cl(s) and 0.368 mol of NH3, the number of moles of HClpresent is moles.

The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g)If an equilibrium mixture of the three compounds in a 6.16 L container at 298 K contains 2.05 mol of NH4HS(s) and 0.359 mol of NH3, the number of moles of H2Spresent is moles.

The equilibrium constant, K, for the following reaction is 5.00x10-2 at 642 K. COCI2(g) : =CO(g) + Cl2(g) An equilibrium mixture of the three gases in a 5.49 L container at 642 K contains 0.288 M COCI2, 0.120 M CO and 0.120 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 11.9 L? [COCI2] = [CO] [Cl2] M ΣΣΣ Il||

The equilibrium constant, Kc, for the following reaction is 0.0952 at 350. K. CH₁ (g) + CCl4 (g) 2CH₂Cl2 (g) Calculate the equilibrium concentrations of reactants and product when 0.205 moles of CH4 and 0.205 moles of CCL are introduced into a 1.00 L vessel at 350. K. [CH4] = | M [CC14] = [CH₂ Cl₂] = M M

The equilibrium constant, Kp , for the following reaction is 1.04×10-2 at 548 K.NH4Cl(s) NH3(g) + HCl(g)If an equilibrium mixture of the three compounds in a 6.28 L container at 548 K contains 1.00 mol of NH4Cl(s) and 0.224 mol of NH3(g), the partial pressure of HCl(g) is  atm.

The equilibrium constant, K, for the following reaction is 9.23×10-3 at 304 K. NH4HS(s) =NH3(g) + H2S(g) An equilibrium mixture in a 18.5 L container at 304 K contains 0.268 mol NH4HS(s), 0.133 M NH3 and 6.94×10-2 M H2S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.86 L? [NH3] = [H2S] = ΣΣ

The equilibrium constant, Kp, for the following reaction is 1.04x102 at 548 K. NH4CI(S) NH3(9) + HCI(g) If an equilibrium mixture of the three compounds in a 5.40 L container at 548 K contains 2.83 mol of NH4Cl(s) and 0.186 mol of NH3(g), the partial pressure of HCI(g) is atm.