0
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2]
Without knowing concentrations, one cannot calculate the actual value of Keq.
What else can I help you with?
What is the correct form for the equilibrium constant expression for this reaction H2g plus F2g 2 HFg?
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.
What are the acids in the following equilibrium reaction cn- plus h2o hcn plus oh?
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-).
The equilibrium constant Kp for the following reaction is 1.57 at 600 K CO(g) plus Cl2(g) COCl2(g) Calculate the equilibrium partial pressures of all species when CO and Cl2 each at an intitial partia?
To calculate the equilibrium partial pressures, we start with the balanced reaction: CO(g) + Cl2(g) ⇌ COCl2(g). Given the initial partial pressures of CO and Cl2 are both ( P_0 ), we can set up an ICE (Initial, Change, Equilibrium) table. At equilibrium, let the change in the concentration of CO and Cl2 be ( -x ), and the change in COCl2 be ( +x ). The equilibrium expression is ( K_p = \frac{P_{COCl2}}{P_{CO} \cdot P_{Cl2}} = 1.57 ). Substituting the equilibrium pressures into the equation and solving for ( x ) allows us to find the equilibrium partial pressures of all species.
What happens to the reaction 2 N O 2 in equilibrium with N 2 O 4 plus 57.3 kilojoules when the temperature of the reaction is increased?
This is an endothermic equilibrium reaction Thus, increase temperature will push the reaction to the right. So more N2O4 is produced
What happends to the OH- as the H plus increases?
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
What is the value of the equilibrium constant at 25 and degC for the reaction between Cr(s) and Cu2 plus (aq)?
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.
What is the equilibrium constant for the reaction h2g plus co2g h2og plus cog?
Keq = [H2O][CO] [H2][CO2]
What is the correct form for the equilibrium constant expression for this reaction H2g plus F2g 2 HFg?
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.
What is the equilibrium constant for the following reaction C plus O CO?
The equilibrium constant for the reaction C + O2 -> CO is Kc = [CO]/([C][O2]), where the square brackets denote molar concentrations.
What is the equilibrium constant of aA plus bB equals cC plus dD?
The equilibrium constant (K) for the reaction aA + bB ⇌ cC + dD is expressed as K = [C]^c [D]^d / [A]^a [B]^b, where square brackets denote the concentrations of the respective species at equilibrium. The coefficients a, b, c, and d correspond to the stoichiometric coefficients of the reactants and products in the balanced chemical equation. The equilibrium constant provides insight into the extent of the reaction and the relative concentrations of reactants and products at equilibrium.
What is the equilibrium constant for the reaction SO2(g) plus NO2(g) --- SO3(g) plus NO(g)?
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.
What is ka for h3bo3(aq) h plus (aq) plus h2bo3-(aq)?
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.
The reaction h2 g plus i2 g 2hi g has keq equals 0.15 at a certain temperature if h2 equals 0.01 i2 equals 0.02 and hi equals 0.03 what is true about this reaction?
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.
What is Keq for the reaction H2(g) plus Cl2(g) 2HCl(g)?
For 2HCl(g) ==> H2(g) + Cl2(g) the Keq = [H2][Cl2]/[HCl]^2
What is the base dissociation constant for a weak base at equilibrium B plus H2O BH plus plus OH?
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].
Is there a pKa value for CO2 plus H2O - H2CO3?
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.
What is k eq for the reaction 2HCI(g) H2(g) plus CI2(g)?
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.
