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Chemical reaction - 0.823 grams O2 could be produced from 2.45 g of ko2 and 4.48 g of CO_2
What is Chemical reaction?
Chemical reactions happen absolutely everywhere. While we sometimes associate chemical reactions with the sterile environment of test tubes and laboratories, nothing is farther from the truth. In fact, a vast number of transformations are creating a dizzying and almost incomprehensible series of new matter and energy changes in our world every second of every day. In nature, chemical reactions can be much more difficult to control and in some cases much more complex than in the laboratory, and generally occur whether you want it or not!In the woods A raging fire, the slow rusting process of iron over the years in the presence of oxygen and water, or the delicate ripening of fruit on a tree, the transformation of various chemicals, etc... (reactants ) into another group of substances (products) is a so-called chemical reaction.
Moles KO2 = 2.44g/(71.1g/mole) = 0.034 moles
Moles CO2 = 4.45g/(44g/mole) = 0.10 moles
4KO2 + 2CO2 —> 2K2CO3 + 3O2
The reaction requires twice as many moles of KO2 than moles of CO2. That means 0.10 mole of CO2 would consume 0.20 moles of KO2. But we only have 0.034 moles of KO2, so the limiting reagent is KO2.
There are 3 moles of O2 produced for every 2 moles of CO2 consumed. In this case we'll assume all of the KO2 reacts, so that should result in (3/4) * (0.034moles) = 0.025 moles of O2 .
To get the mass, 0.025 mole * (32g/mole) = 0.823 grams O2
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