Consider the following reaction and its equilibrium constant K: 3.45 X 10-2 Smol-1:
NH3 + HCl ⇌ NH4Cl
If concentration for reactants are given as following:
[NH3] = 0.20 M;
[HCl] = 0.45 M
Determine the concentration of NH4Cl in this reaction.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Consider the following reaction and its equilibrium constant K: 3.45 X 10-2 Smol-1: NH3 + HCl...
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 0.208 mol NH4Cl, 2.26×10-3 M NH3 and 2.26×10-3 M HCl. If the concentration of HCl(g) is suddenly increased to 3.80×10-3 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = M [HCl] = M
(1). The equilibrium constant, K, for the following reaction is 1.32×10-3 at 565 K. NH4Cl(s) =NH3(g) + HCl(g) An equilibrium mixture in a 10.4 L container at 565 K contains 0.285 mol NH4Cl(s), 4.47×10-2 M NH3 and 2.95×10-2 M HCl. 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 4.25 L? [NH3] = M [HCl] = M
-The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.452 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCl] = _________M -The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g) + I2(g) 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H2and 0.380 moles of I2are introduced into a 1.00...
The equilibrium constant, K, for the following reaction is 2.57×10-4 at 549 K. NH4Cl(s) NH3(g) + HCl(g) An equilibrium mixture in a 14.3 L container at 549 K contains 0.321 mol NH4Cl(s), 1.97×10-2 M NH3 and 1.30×10-2 M HCl. 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 6.96 L? [NH3] = __________M [HCl] = ___________M
Consider the following reaction: NH4Cl(s) -->NH3(g) + HCl(g) If a flask maintained at 560 K contains 0.191 moles of NH4Cl(s) in equilibrium with 3.79×10-2 M NH3(g) and 2.11×10-2 M HCl(g), what is the value of the equilbrium constant at 560 K? K =
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 5.41 L container at 548 K contains 1.17 mol of NH4Cl(s) and 0.350 mol of NH3, the number of moles of HCl present 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...
The equilibrium constant, Kc, for the following reaction is 5.0110 at 514 K. NH4Cl(s) =NH3(g) + HCl(g) Calculate Ke at this temperature for the following reaction: NH3(g) + HCI(g) = NH,Cl(s) K. = ) Submit Answer Retry Entire Group 1 more group attempt remaining
The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s)----> NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.388 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.46×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = ______ M [HI] = _______ M
The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) -->NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.335 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.28×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...