40 POINTS!! Will Mark Brainliest if all work is shown as well as correct answer The following reaction can be used to convert carbon dioxide to oxygen gas.

4 KO₂ (s) + 2 CO₂(g) → 2 K₂CO₃(s) + 3 O₂(g)

The theoretical yield for the reaction is 0.296 g O₂. Given that the reaction has a percent yield of 83.4%, what is the mass in g of oxygen gas that is actually produced?

0.3549

Explanation:

the percentage yield is the percentage of the product formed based on the theoretical yield.in this question the percentage yield and theoretical yield have been given all that's left is the actual yield.so you use the formula

percentage yield=theoretical yield/actual yield×100

83.4=0.296/ay×100

83.4ay/83.4=100×0.296/83.4

ay=0.3549

I hope this helps

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.