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.
We know
Change in no. of moles = (total no. of moles of products) - (total no. of moles of reactants)
In the following reaction, the initial concentrations of the reacting mixture contains the [H2O] = 1.00...
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.
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?
For the reaction H2O(g)+Cl2O(g)<->2HOCl, K=0.900 at 25 degrees Celsius. What are the equilibrium concentrations of each species beginning with 0.300 M of each reactant? Complete the ICE table Solve for the equilibrium concentrations asked for Briefly describe what simplification would be needed to complete the question
Find the equilibrium concentration of HOCI in the decomposition equilibrium reaction if the initial concentrations of H20 and Cl20 are both 0.980 M, and that Kc = 0.0900. 2HOCI(g) = H2O(g) +C120(g)
3) The value of Kc for the reaction between water vapor and dichlorine monoxide, H2O(g) + Cl20 (g) = 2 HOCI (g) is 0.0900 at 25°C. Determine the equilibrium concentrations of all three compounds if the starting concentrations of both reactants are 0.00432 M and no HOCI is present.
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
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is H2(g) + I2(g) --> 2HI (g) What is the value of Kc? What is the value of Kp?
For the following reaction, the initial concentrations of CO is 0.500M and Cl2 is 1.00 M. What are the equilibrium concentrations of each species at 400K? (show all work) COCl2(g) ⇌ CO(g) + Cl2 (g) Kc = 0.680 at 400 K
Calculate the concentrations of all substances present in the equilibrium mixture, if 2.35 mol of H2 and 2.35 mol of I2 are placed in a 10.0 L flask and allowed to come to equilibrium, at which time 3.76 mol of HI are present. The reaction is b) What is the value of Kc? c) What is the value of Kp
1A) A mixture initially contains A, B, and C in the following concentrations: [A] = 0.300 M , [B] = 1.15 M , and [C] = 0.400 M . The following reaction occurs and equilibrium is established: A+2B⇌C At equilibrium, [A] = 0.190 M and [C] = 0.510 M . Calculate the value of the equilibrium constant, Kc. 1B) Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make...