SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2]
Without knowing concentrations, one cannot calculate the actual value of Keq.
The correct form for the equilibrium constant expression for this reaction is Kc = [HF]^2 / ([H2] * [F2]), where the square brackets denote molar concentrations of each species at equilibrium.
The acid in the reaction is hydrogen cyanide (HCN), which is formed when cyanide ion (CN-) reacts with water (H2O) to release hydroxide ion (OH-).
This is an endothermic equilibrium reaction Thus, increase temperature will push the reaction to the right. So more N2O4 is produced
The concentration of OH- decreases as the concentration of H+ increases. This is beacause there is an equilibrium H2O <-> H+ + OH- and therefore the [H+][OH-] is a constant
A catalyst would increase the rate of the reaction by providing an alternative pathway with lower activation energy. This would allow the reaction to occur more quickly without being consumed in the process. The equilibrium concentrations of the reactants and products would remain the same.
The equilibrium constant for the reaction between Cr(s) and Cu2+ (aq) cannot be determined without knowing the specific reaction equation. The equilibrium constant (K) is a unique value for each specific reaction at a given temperature.
Keq = [H2O][CO] [H2][CO2]
The correct form for the equilibrium constant expression for this reaction is Kc = [HF]^2 / ([H2] * [F2]), where the square brackets denote molar concentrations of each species at equilibrium.
The equilibrium constant for the reaction C + O2 -> CO is Kc = [CO]/([C][O2]), where the square brackets denote molar concentrations.
The equilibrium constant for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) is given by the expression Kc = [SO3][NO]/[SO2][NO2], where square brackets denote molar concentrations. The numerical value of this equilibrium constant would depend on the specific conditions of the reaction.
The equilibrium constant expression for the reaction you provided would be ( K_a = \frac{[H^+][H_2BO_3^-]}{[H_3BO_3]} ). However, the specific value of ( K_a ) for this reaction would depend on the concentrations of the species involved in the particular experimental conditions.
This reaction is not at equilibrium yet since the reaction quotient, Q, is not equal to the equilibrium constant, K. In this case, Q = (0.03)^2 / ((0.01)*(0.02))^2 = 0.45, which is greater than K = 0.15. Therefore, the reaction will proceed in the reverse direction to reach equilibrium.
For 2HCl(g) ==> H2(g) + Cl2(g) the Keq = [H2][Cl2]/[HCl]^2
The base dissociation constant (Kb) is a measure of the strength of a weak base. It is defined as the ratio of the concentrations of the products (BH+ and OH-) to the concentration of the reactant (B) at equilibrium. Mathematically, Kb = [BH+][OH-]/[B].
Yes, the pKa value for the reaction of CO2 plus H2O to form H2CO3 is approximately 6.35. This represents the equilibrium constant between the dissolved CO2 and H2CO3 forms in water.
The equilibrium constant (K eq) for the reaction 2HCl(g) ⇌ H2(g) + Cl2(g) would be [H2][Cl2]/[HCl]^2, where the square brackets indicate the molar concentrations of the respective species at equilibrium.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.