H2s(g) is an endothermic process. a 6.1589−g sample of the solid is placed in an evacuated 4.000−l vessel at exactly 24°c. after equilibrium has been established, the total pressure inside is 0.709 atm. some solid nh4hs remains in the vessel. (a) what is the kp for the reaction? (b) what percentage of the solid has decomposed? % (c) if the volume of the vessel were doubled at constant temperature, what would happen to the amount of solid in the vessel? more than 50% would remain. between 20% and 50% would remain. between 10% and 20% would remain. less than 10% would remain.

Answer asap need by wednesday morning explain how a buffer works, using an ethanoic acid/sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.

The characteristics of two different types of reactions are shown below: reaction a: electrons are gained by the atoms of an element. reaction b: protons are lost by the atom of an element. which statement is true about the atoms of the elements that participate in the two reactions? their identity changes in both reaction a and reaction b. their identity changes in reaction a but not in reaction b. their identity changes in reaction b but not in reaction a. their identity remains the same in both reaction a and reaction b.

How can the periodic table be used to predict the behavior of elements?