Given 3.4 grams of x compound with a molar mass of 85g and 4.2 grams of y compound with a molar mass of 48g How much of compound xy can be generated 2x + Y2 = 2xy

Answer 1

There is a little confusion here when you refer to "compound" X and Y. Not so much with X, but since you have Y₂, that could be something like Cl₂ (a compound), but then Y would be Cl (an element) and not a compound. So, I'm assuming when you say "4.2 grams compound Y with molar mass 48 g" you mean compound Y₂. If that's not the case, you need to re-submit the problem with clarity. Or tell whoever wrote the problem to write it more clearly.

2X + Y₂ ==> 2XY

moles X present = 3.4 g x 1 mol / 85 g = 0.04 moles X

moles Y₂ present = 4.2 g x 1 mol / 48 g = 0.0875 moles Y2

Limiting reagent is X because it takes 2 of X for each 1 of Y₂ and clearly we don't have that mol ratio here.

The limiting reagent will dictate how much product can be formed, so to find how much XY is formed, we have....

(0.04 moles X)(2 mol XY/2 mol X) = 0.04 moles XY

If you want the answer in grams, you need to use molar mass of XY and that would be

X = 85

Y = 1/2 x 48 = 24

molar mass = 109 g/mol

109 g/mol x 0.04 moles = 4.4 g XY