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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?
Q = [.125]2 / [.417][.531]3
Identify the metal used as the catalyst in the Haber process?
its Fe- iron. It is used as a catalyst to speed up the exothermic reaction between N2 and H2 to make NH3.
What is the k in the rate law equation?
A rate constant
The reaction quotient Q indicates?
Q indicates wether or not a reaction will occur when the value of Q is compared to the equilibrium constant K if Q is larger than K the reaction will occur from product to reactant (decomposition) if Q is smaller than K the reaction will occur from reactant to product
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)
Which of the following is the equilibrium constant of a reaction?
Keq = products/reactions
What does it mean if keq1?
I suspect it could be " k eq 1" , or "k =1".
What is k eq for the reaction 2HCI(g) H2(g) plus CI2(g)?
For the reaction 2HCl(g) ==> H2(g) + Cl2(g), the Keq = [H2(g)][Cl2(g)]/[HCl(g)]^2
What does K value of approximately 1 show about the equilibrium?
If the K is as much as 1.3 then the reaction is running to product.
What is the rate of a reaction that follows the rate law rate kAmBn where k 0.2 A3 M B3 M m1 n2?
answer is 5.4 (mol/L)/s
What is an expression of Boyle's law (k constant)?
PV=k Apex (:
0.417 M N2 0.531 M H2 and 0.125 M NH3 at 800 K Kc equals 0.278 calculate the reaction quotient?
Q = [.125]2 / [.417][.531]3
How can a chemical equation be used to write a equilibrium-constant expression?
In the equilibrium system: aA + bB <=> cC + dD [A]a x [B]b K = ___________ [C]c x [D]d Where A, B, C and D are gases or solutions. Pure liquids and solids are not included in the equilibrium constant expression.
