If you reverse an equation, why is the equilibrium constant (Kc or Kp) inverted?
A (aq) + B (aq) ←→ C (aq) + D (aq)K = ([C][D])/([A][B])C (aq) + D (aq) ←→ A (aq) + B (aq)K prime = ([A][B])/([C][D])Now you see that the law of mass action will always have the products in the numerator and the reactants in the denominator. When you reverse the reaction, these two switch places. Therefore:K = 1/K prime
At 850 K, the equilibrium constant for the following equation is Kc=15.?
From the Law of Mass Action, the equilibrium constant for this reaction is defined as: Kc = [SO3]² / [SO2]² [O2] = 15.0 The Reaction Quotient, Qc, is calculated exactly the same way from the given reaction mixture concentrations. Just substitute the given concentrations. If Qc = Kc, the reaction mixture is in equilibrium. If Qc > Kc, the reaction will shift to the left. If Qc < Kc, the reaction will shift to the right. For the above mixtures, Qc = 15 for the top, 40.8 for the middle, and 0.08 for the bottom. Therefore the top mixture is in equilibrium, the middle will shift to the left, and the bottom will shift to the right.
The equilibrium constant Kc for the reaction:?
The equilibrium constant Kc for the reaction: 2HCL(g)<---->H2(g)+Cl2(g) is 4.17 X10^-34 at 25 degrees C. What is the equilibrium constant for the reaction H2(g)+Cl2(g) <---->2HCl(g) at the same temperature.. I do not understand any of this. please help!
What's the Arrhenius Equation variation for equilibrium constant?
First of all, you wrote down a mix up of equations, probablyThe Arrhenius Equation writes down as[math]k = Ae^-{E_a}/RT[/math]withA is some constantEa is the activation energyR is the universal constant of gasesT is the absolute temperatureThis equation relates the dependence of the K (equilibrium constant) with the temperature.Thinking only at the mathematical aspects, this equation ensures that the greater is the temperature, the greater is the equilibrium constant, since the exponential that have the temperature as a factor in the denominator but showing a minus sign in the exponential. Thus, as T increases, [math]{E_a}/RT[/math] decreases and the factor [math]-{E_a}/RT[/math] increases, resulting in a increased above mentioned.
Finding Equilibrium Constant?
2. If the value of Kb for pyridine (C5H5N) is 1.8x10-9 at 298 K, calculate the equilibrium constant, Ka, for the reaction C5H5NH+(aq) + H2O(l) <--> C5H5N(aq) + H30+(aq). I have no real clue where to go with this, could someone please help?
Given the following below find the equilibrium constant for N2 + 1/2 O2 --><-- N2O?
When using multiple equations to calculate a new Kc, there are a few general rules. If you flip an equation around, you take the reciprocal of Kc. When you add two equations, you multiply their Kc's together. So, Start by flipping your first equation over to give: 2 NO <--> N2O + 1/2 O2 Kc = 1/1.7X10^-13 = 5.9 X 10^12 Then just add that to the second equation, canceling terms, and multiply the two Kc's together: 2 NO <--> N2O + 1/2 O2 Kc = 5.9 X 10^12 N2 + O2 <--> 2 NO Kc = 4.1 X 10^-31 ______________________________________... N2 + 1/2 O2 <--> N2O Kc = 2.4 X 10^-18
How to find equilibrium constant for the reverse reaction?
I encountered a question where it only gives the balanced equation, temperature, and Keq (equilibrium constant) value. No values for concentration or any value that could be used to calculate concentration were given, so I don't think I could use the usual formula for Keq ([reactants]/[products]). Can anyone help me? Here's the specific question, if it would help: Given : Temperature : 1500 degrees Celcius Equilibrium Constant : 0.1764 Balanced equation: CO + 3 H2 <=>CH4 + H2O Need: Equilibrium Constant for CH4 + H2O <=> CO + 3H2