Acetic acid is the active ingredient in vinegar. in a solution of acetic acid the following equilibrium is established. hc2h3o2(aq) < --> h+(aq) + c2h3o2-(aq) the equilibrium constant for this reaction is 1.8 x 10–5. what is the equilibrium constant for the following reaction ? h+(aq) + c2h3o2-(aq) < --> hc2h3o2(aq)

the equilibrium constant is 1.8 x 10⁻5 and strongly favor the reactants.

Explanation:

the chemical reaction provided for the two equation are the same but different direction i.e a reversible reaction. Assuming, the mass of reactants and product and temperature remain constant.

therefore, the equilibrium constant K, is 1.8 x 10⁻5. this is a very small value of K, thereby strongly favor the backward direction to form reactant.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

where's the diagram?