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What does it mean if k eq 1?
reactants are favored over products in the reaction
0.417 M N2 0.531 M H2 and 0.125 M NH3 at 800 K Kc equals 0.278 calculate the reaction quotient?
To calculate the reaction quotient Qc, use the formula Qc = [NH3]^2 / ([N2]*[H2]). Substitute the given concentrations into the equation: Qc = (0.125^2) / (0.417 * 0.531) ≈ 0.087.
What are the units for the equilibrium constant k?
I'm taking an awesome chemistry final tomorrow. So, I'm not a massive failure at this: k=mol/liters Kc can only determine by experiment , not by evaluations of equations. so when writting the eq of Kc= [] products /[reactants], do not use units for [], as Kc has no units. Kc, only affected by temperature...
What is the k in the rate law equation?
A rate constant
What is the balanced reaction between ethanol and potassium?
The balanced reaction between ethanol (C2H5OH) and potassium (K) is 2C2H5OH + 2K --> 2C2H5OK + H2. This reaction forms potassium ethoxide and hydrogen gas as products.
What is keq for the reaction n2 3h2 2nh3 if the equilibrium concentrations are nh3 2 m n2 3 m and h2 1 m?
K(eq)= 1.33
What does it mean if K eq?
reactants are favored over products in the reaction
What does it mean if k eq 1?
reactants are favored over products in the reaction
What is the Derivative of y equals k multiplited by N divide 1 plus N2 where k is a constant?
y = kn / (1 + n2)First, let's express it with negative exponents:y = kn * (1 + n2)-1Then apply the chain rule:dy|dn = k(1 + n2)-1 - kn(1 + n2)-2 * 2nAnd simplify:dy|dn = k / (1 + n2) - 2n / kn(1 + n2)
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.
What does it mean if keq1?
I suspect it could be " k eq 1" , or "k =1".
Which of the following is the equilibrium constant of a reaction?
Keq = products/reactions
What is an expression of Boyle's law (k constant)?
PV=k Apex (:
What is the balanced equation of nitrogen gas with oxygen gas to produce nitrogen monoxide at an equilibrium constant?
The balanced equation for the reaction between nitrogen gas and oxygen gas to produce nitrogen monoxide is: 2N2(g) + O2(g) ⇌ 2NO(g) The equilibrium constant for this reaction would be expressed as K = [NO]^2 / [N2]^2[O2].
0.417 M N2 0.531 M H2 and 0.125 M NH3 at 800 K Kc equals 0.278 calculate the reaction quotient?
To calculate the reaction quotient Qc, use the formula Qc = [NH3]^2 / ([N2]*[H2]). Substitute the given concentrations into the equation: Qc = (0.125^2) / (0.417 * 0.531) ≈ 0.087.
What does K value of approximately 1 show about the equilibrium?
A K value of approximately 1 indicates that the concentrations of products and reactants at equilibrium are roughly equal. This suggests that the reaction is proceeding in both the forward and reverse directions at similar rates, resulting in a dynamic equilibrium.
How can a chemical equation be used to write a equilibrium-constant expression?
Law of mass action (also called 'Law of Guldberg & Waage')Generalized reaction equation (cf. Note): aA + bB pP + qQAccording to the Law of mass action:Equilibrium constant (K>/) and backward (
