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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?
The units for the equilibrium constant, K, depend on the specific reaction. However, K is dimensionless for gases, while for reactions involving concentrations, the units of K will depend on the stoichiometry of the reaction.
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 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 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 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.
How can a chemical equation be used to write a equilibrium-constant expression?
A chemical equation can be used to write an equilibrium constant expression by taking the concentrations of products raised to their stoichiometric coefficients and dividing by the concentrations of reactants raised to their stoichiometric coefficients. The equilibrium constant expression is written in terms of the molar concentrations of the species involved in the reaction.
Calculate delta G at 298K for the reaction of nitrogen and hydrogen to form ammonia of the delta G equals -33.3kJn and the reaction mixture consists of the follwing N2.5 atms H2.75 NH3 2.0?
Given that the reaction is N2(g) + 3H2(g) → 2NH3(g), the existing equilibrium constant K at 298K can be calculated using the given partial pressures of N2, H2, and NH3. Then, using the equation ΔG = -RT * ln(K), we can find the Gibbs free energy change. Subtituting the values, we would get ΔG = -33.3kJ/mol.
