Write the equilibrium constant expression, K, for the following reaction. Please

Question

Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 HNO2 (aq) + H2O(l) H3O+(aq) + NO2- (aq) K = Bromine is one of the few elements that is a liquid at room temperature. It vaporizes easily and has a beautiful red color in both the liquid and gaseous states. Bromine reacts readily with hydrogen gas to make hydrogen bromide. One way to represent this equilibrium is: HBr(g) 1/2 H2(g) + 1/2 Br2(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are released. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. Witte the K1 expression for an aqueous solution of hypochlorous acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator the top box and the complete denominator on the bottom box. Remember to write the hydonium ion out as H3O+, and not at H+)

Explanation / Answer

Question 1.

K = [Products]^p / [reactants]^r

then

K = [H3O+][NO2-]/([HNO2][H2O])

since H2O is liquid, then activity = 1

K = [H3O+][NO2-]/([HNO2])

Q2.

H2(g) + Br2(g) <-> 2HBr(g)

Kp = P-HBr^2 / ((P-H2)(P-Br2))

Kp = inverted and powered to second

Kp = (Kp1)^-2

Q3.

this is just inverted so

Kp = (Kp1)^-1

Q4.

this is just multiplied by two, implies power to second

Kp = (Kp1)^2

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