The equilibrium constant, K, for the following reaction is 5.10×10-6 at 548 K. NH4Cl (s) NH3 (g) + HCl (g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.396 mol NH4Cl, 2.26×10-3 M NH3 and 2.26×10-3 M HCl. If the concentration of NH3(g) is suddenly increased to 4.09×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

The equilibrium constant, K. , for the following reaction is 1.80x10 at 298 K. NH,HS(s) NH3(g)+ H,S(g) If an equilibrium mixture of the three compounds in a 6.85 L container at 298 K contains 1.56 mol of NH HS(s) and 0.468 mol of NH3, the number of moles of H,S present is moles.

The equilibrium constant, K, for the following reaction is 1.80×10-2 at 510 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 7.99 L container at 510 K contains 0.377 M PCl5,   8.23×10-2 M PCl3 and 8.23×10-2 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 18.5 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl(g) COCI,(g) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of CO and 0.451 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] [Cl] [COCL,] = MMM

The equilibrium constant, K, for the following reaction is 5.39×10-3 at 680 K. NH4I (s)  NH3 (g) +  HI (g) An equilibrium mixture in a 18.7 L container at 680 K contains 0.270 mol NH4I(s), 9.62×10-2 M NH3 and 5.60×10-2 M HI. 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 10.1 L? [NH3] =  M [HI] =  M

The equilibrium constant, K, for the following reaction is 3.46x102 at 630 K. COCI₂(g) CO(g) + Cl₂(g) An equilibrium mixture of the three gases in a 11.8 L container at 630 K contains 0.217 M COCI₂, 8.67x10-2 M CO and 8.67x10-2 M Cl₂. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 4.74 L? [COCI₂] = [co] [Cl₂] = M ΣΣ

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.

A chem ngineer is studying the following reaction: 4 HCl(g)+O,(g) – 2 H,0(g)+2Cl,(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 0.0040. The engineer charges ("fillsf) four reaction vessels with hydrogen chloride and oxygen, and lets the reaction begin. He then measures the co mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction compound pressure expected change in pressure vessel HCl 8.71 atm Ot increase O! decrease O (no change) 02 8.13 atm O t increase OI decrease O (no change) H,0 3.63 atm Ot increase OI decrease (no change) I decrease (no change) Cl, 1.91 atm ease I decrease (no change) 7,61 atm t increase HCI I decrease O (no change) 7,86 atm O f increase 0, I decrease O (no change) 4.18 atm t increase H,0 I decrease (no change) t increase 2.46 atm Cl, I decrease O (no…

The equilibrium constant, K, for the following reaction is 5.10x10 at 548 K. NH4Cl(s) NH3(g) + HCI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.368 mol NH4Cl, 2.26x10-3 M NH₂ and 2.26×10-³ M HCl. If the concentration of HCl(g) is suddenly increased to 3.22×103 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH₂] = [HCI] M M

The equilibrium constant, K, for the following reaction is 1.32x10-3 at 565 K. NH4CI(S) NH3(g) + HCI(g) An equilibrium mixture in a 10.0 L container at 565 K contains 0.333 mol NH4Cl(s), 4.54x10-2 M NH3 and 2.91x10-² M HCI. 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 4.36 L? [NH3] = [HCI] = Submit Answer M M Retry Entire Group 8 more group attempts remaining