Achemist reacted 17.25 grams of sodium metal with excess chlorine gas. the chemical reaction is as follows

na + cl2 → nacl

if the percentage yield of the reaction is 88%, what is the actual yield?

38.588 g ≅ 35.60 g.

Explanation:

Using cross multiplication:

2.0 moles of Na metal produce → 2.0 moles of NaCl,

∴ 0.75 mole of Na metal produce → 0.75 mole of NaCl.

∵ The percentage yield = [(actual yield) / (calculated yield)] x 100.

∴ The actual yield = [(the percentage yield)(calculated yield)] / 100 = [(88 %)(43.85 g)] / 100 = 38.588 g ≅ 35.60 g.

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation:

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