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Consider this reaction: 4 KO2 (s) + 2 CO2 (g) ? 2 K2CO3(s) + 3 O2(g)
(a) How many moles of oxygen gas are produced when 0.400 mol of KO2reacts with excess carbon dioxide?
(b) How many grams of KO2 are needed to form 7.50 g of oxygengas?
(c) How many grams of CO2 are used when 7.50 g of oxygen areproduced?

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Keith Leannon
Keith LeannonLv2
28 Sep 2019
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Related questions

Consider the reaction 4 KO2(s) + 2 CO2(g) รขย†ย’ 2 K2CO3(s) + 3 O2(g). How much oxygen is produced at STP if 10.5 moles of carbon dioxide are used at STP?

Please show work

Potassium superoxide, KO2, is often used in oxygen masks (such as those used by firefighters) because KO2 reacts with CO2 to release molecular oxygen. Experiments indicate that 2 mol of KO2(s) react with each mole of CO2(g). (a) The products of the reaction are K2CO3(s) and O2(g). Write a balanced equation for the reaction between KO2(s) and CO2(g). (b) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced? (c) What mass of KO2(s) is needed to consume 18.0 g CO2(g)? What mass of O2(g) is produced during this reaction?

Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and dioxygen as follows: 4KO2+ 2CO2 -> 2K2CO3 + 3O2. This reaction makes potassium superoxide useful in a self-contained breathing apparatus.

a) Given th balance chemical equaition above, what is the mole relationship between KO2 and O2?

b)If you started with 0.250 mole of KO2 and 0.250 moles of CO2, which is your limiting reagent?

c) If an apparatus contains 2.50g KO2, how many grams of O2 is produced?

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