H2O(g) + Cl2O(g) -------------> 2 HOCl(g)
Start 0 0 1.5
Change +x +x -2x
Equil. +x +x 1.5-2x
Kc = [HOCl]^2/[H2O][Cl2O]
0.09 = (1.5-2x)^2/x*x
0.09 = (1.5-2x/x)^2
0.3 = 1.5-2x/x
0.3x = 1.5-2x
x = 0.652
[H2O] = x = 0.652M
[Cl2O] = x = 0.652M
[HOCl] = 1.5-2x = 1.5-2*0.652 = 0.196M
At 25oc, Kc = 0.090 for the following reaction. H2O(g) + Cl2O(g) 2 HOCl(g) Calculate the...
1. At 25oc, Kc = 0.090 for the following reaction. H2O(g) + Cl2O(g) 2 HOCl(g) Calculate the equilibrium concentration of all species if the initial concentration of HOCl = 1.50 M. H2O(g) + Cl2O(g) 2 HOCl(g) Start Change Equil.
Consider the following reaction and the value of its equilibrium constant: H2O(g) + Cl2O(g) ⇌ 2HOCl(g) Keq = 0.090 If the equilibrium concentration of HOCl is measured at 0.15 M, what are the equilibrium concentrations of H2O and Cl2O, assuming that they are equal?
H2o+cl2o.....>2hocl Starting conc for h20 and cl2o is 0.0032 M and the equilibrium concentration for hocl is 0.0012M. What is value of equilibrium constant.
For the following process: H2O(g) + Cl2O(g) à 2HOCl(g) Ho(H2O(g))= 242KJ/mol Ho(Cl2O(g))=80KJ/mol Ho(HOCl(g))= -80KJ/mol So(H2O(g))= 0.189 KJ/K So(Cl2O(g))=0.266 KJ/K So(HOCl(g))= 0.237 KJ/K A) Calculate ΔHo, ΔSo and ΔGo B)Calculate ΔG at 100K and P(H2O)=P(Cl2O)= P(HOCL)=10atm
For the following reaction: HA(aq) + H2O(l) ⇌ H+(aq) + A-(aq), Kc = 2x10-7 at 25oC The initial concentration of [HA] = 0.50M. What is the [H+] of the solution at equilibrium? Hint: you can assume x is small in comparison to 0.5M.
A mixture of 0.482 M H20, 0.419 M Cl20, and 0.748 M HCIO are enclosed in a vessel at 25 °C. (Reaction) H2O(g) + C12O (g) <------> 2HOCI(g) Kc = 0.090 at 25 °C Calculate the equilibrium concentrations of each gas at 25 °C [H2O] = M [Cl2O] = M [HOCL]= M
At 25°C, K = 0.090 for the following reaction. H20(g) Cl20(g)2 HOCI(g) Calculate the concentrations of all species at equilibrium for each of the following cases. (a) 1.3 g H20 and 2.0 g Cl20 are mixed in a 1.1-L flask. [Cl20] [H2O] 四 (b) 1.5 mol pure HOCI is placed in a 1.7-L flask Cl20] [H2O]
In the following reaction, the initial concentrations of the reacting mixture contains the [H2O] = 1.00 M and [Cl2O] = 1.00 M at 25 deg C. The mixture is allowed to come to equilibrium. H2O(g) + Cl2O(g) <=> 2HOCl(g) ; Kc = 0.0900 Determine the Kp value of the reaction.
A mixture of 0.505 M H2O , 0.378 M Cl2O , and 0.747 M HClO are enclosed in a vessel at 25°C . H2O(g)+Cl2O(g)−⇀↽−2HOCl(g)Kc=0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25°C . A mixture of 0.505 M H,0,0.378 M C1,0, and 0.747 M HCIO are enclosed in a vessel at 25°C. H2O(g) + C1,0(g) = 2 HOCI(g) Kc = 0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C.
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.72 mol H2 and 0.72 mol CO2 are injected into a 4.5−L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: M Equilibrium concentration of CO2: M Equilibrium concentration of H2O: M Equilibrium concentration of CO: M