The equilibrium constant expression for the reaction is Kc = [H2O]^2/[SO2][O2]. Given the concentrations at equilibrium, we can solve for [H2O]. Plugging in the values, we get 31.25 = [H2O]^2 / (0.03)(0.05). Solving for [H2O] gives us [H2O] = sqrt(31.25 * 0.03 * 0.05), which is approximately 0.275M.
Given the equilibrium constant (Kc) is 0.625 and the concentrations of O2 and H2O at equilibrium are 0.40 and 0.20 respectively, you can use the equilibrium expression Kc = [H2O2] / ([O2] * [H2O]) to solve for the equilibrium concentration of H2O2. Plugging in the values, you can calculate the concentration of H2O2 at equilibrium.
The equilibrium constant (Kc) for the reaction would be [O2]/([H2O2]^[H2O]) = 0.25/(0.15*0.21) = 7.94
The equilibrium constant (Kc) for a reaction can be calculated using the concentrations of the products and reactants at equilibrium. In this case, Kc = [O2]/([H2O]^2). Plugging in the given values, Kc = (0.92)/((0.37)^2) ≈ 6.56.
The rate constant is independent of the concentration of reactants. It is a constant that reflects the intrinsic characteristics of the reaction. The rate of reaction, on the other hand, is directly proportional to the concentration of reactants raised to the power of their respective stoichiometric coefficients.
The half-life of a first-order reaction is constant because it is based on the rate constant, which is independent of the initial concentration of the reactant. In a first-order reaction, the rate of the reaction is directly proportional to the concentration of the reactant, so as the concentration decreases, the rate of reaction also decreases to maintain a constant half-life period.
To find the equilibrium concentration of NO, first calculate the equilibrium constant expression using the given concentrations of O2 and N2. Then, rearrange the equilibrium constant expression to solve for the concentration of NO. Finally, substitute the values of O2 and N2 concentrations into the rearranged expression to find the equilibrium concentration of NO.
Given the equilibrium constant (Kc) is 0.625 and the concentrations of O2 and H2O at equilibrium are 0.40 and 0.20 respectively, you can use the equilibrium expression Kc = [H2O2] / ([O2] * [H2O]) to solve for the equilibrium concentration of H2O2. Plugging in the values, you can calculate the concentration of H2O2 at equilibrium.
The reaction is: 2H2O2(l) -> 2H2O(l) + O2(g). Using the equilibrium constant expression K = [O2]^2 / [H2O2]^2, you can substitute the given values to calculate [H2O2]. Rearranging the equation gives [H2O2] = sqrt([O2]^2 / K) = sqrt(0.40^2 / 0.625) = 0.32 mol/L. Thus, the equilibrium concentration of H2O2 is 0.32 mol/L.
The equilibrium constant (Kc) for the reaction would be [O2]/([H2O2]^[H2O]) = 0.25/(0.15*0.21) = 7.94
0.28
0.34
The equilibrium constant (Kc) for a reaction can be calculated using the concentrations of the products and reactants at equilibrium. In this case, Kc = [O2]/([H2O]^2). Plugging in the given values, Kc = (0.92)/((0.37)^2) ≈ 6.56.
Using the equilibrium constant expression, (K = \frac{[products]}{[reactants]}), we can set up the equation as (0.62 = [H2O2] / ([O2] * [H2O])). Plugging in the given values, we get (0.62 = [H2O2] / (0.4 * 0.2)). Solving for [H2O2], we find the equilibrium concentration of H2O2 to be 0.62 * 0.4 * 0.2 = 0.0492.
The rate constant is independent of the concentration of reactants. It is a constant that reflects the intrinsic characteristics of the reaction. The rate of reaction, on the other hand, is directly proportional to the concentration of reactants raised to the power of their respective stoichiometric coefficients.
H2(g) + I2(g) 2HI(g)18.6
96
The half-life of a first-order reaction is constant because it is based on the rate constant, which is independent of the initial concentration of the reactant. In a first-order reaction, the rate of the reaction is directly proportional to the concentration of the reactant, so as the concentration decreases, the rate of reaction also decreases to maintain a constant half-life period.