So how much oxygen did we may? It's quite reactive, which is why this reaction works. 0.102250 mole of CO2 would react completely with (4/2) x 0.102250 = 0.2045 moles of KO2, but there is not that much KO2 present, so KO2 is the limiting reactant. Potassium superoxide, KO2, is used for producing oxygen and removing carbon dioxide in selfcontained breathing units, space shuttles, and other enclosed spaces. And here I like to show the units because now we're reassuringly the grandes cancel. 17. If the price of fuel is $2. To see how... broadband telecommunications technology and management book ch Oxygen for First Responders In self-contained breathing devices used by first responders, potassium superoxide, KO9, reacts with exhaled carbon dioxide to produce potassium carbonate and oxygen: 4 KO2s) 2 CO2g)2 K9CO3(s)+3 O2(g) How much O9 could be produced from 85g KOg? So C n is mass divided by molecular weight says what we want to do right now. This reaction makes potassium superoxide useful in a We know we wanted a number Ingram's and that gives us. answer according to text book is 29 g of O2 produced from 85g Oxygen for First Responders In self-contained breathing devices used by... Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and... 7.37. Spell out the full name of the compound.. (FW 149.087 g/mole) is... Iron ore is impure $\mathrm{Fe}_{2} \mathrm{O}_{3} .$ When $\mathrm{Fe}_{2} \mathrm{O}_{3}$ is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. So now we need mass equals and times molecular weight, and that's just 3.0 times 32. As stated in the chapter, potassium superoxide $\left(\mathrm{KO}_{2}\right)$ is a useful source of oxygen employed in breathing equipment. Still have questions? What is the mass percent $\mathrm{Fe}_{2} \mathrm{O}_{3}$ in the ore sample, assuming that none of the impurities contain Fe? (a) Write an equation for the reaction. It looks like this, but scientific notation is a more communion notation in general when you start getting lots of decimal places, okay, so how many moles of Ko to are we consuming? It produces potassium carbonate and oxygen.
Now, from the equation, 2571 g KO2 - 48 g 02 2.45 g KO 48 X 2 .45 2 x 71 = 0.828 g Therefore, mass of O₂ formed = 0.828 g. A self-contained breathing apparatus uses canisters of potassium Please explain step by step, thank you! in this problem, we have the reaction between potassium super oxide and carbon dioxide. Go to your Tickets dashboard to see if you won! Or for bulls times the molecular weight 71.1 And that's in grams per mole and happily are moles. self-contained breathing apparatus. How much $\mathrm{O}_{2}$ could be produced from $2.50 \mathrm{g}$ of $\mathrm{KO}_{2}$ and $4.50 \mathrm{g}$ of $\mathrm{CO}_{2} ?$. POTASSIUM SUPEROXIDE KO2. If the oxygen supply becomes limited or if the air becomes poisoned, a worker can use the apparatus to breath. 4 KO2(s) + 2 CO2(g) - 2 K2CO3(s) + 3 O2(g) Calculate the mass of KO2 reacted if 355.8 mL of gas is collected over water at 65.0 °C and a barometric pressure of 744.8 torr. (a) Write equations for these two reactions and comment on the effectiveness of potassium superoxide in this application. structure of CH3CHCH2CH2CH3, with a –CH3 group attached to the second (from left to right) carbon. First the potassium superoxide reacts with moisture to release oxygen and produce potassium hydroxide. Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen: This reaction makes potassium superoxide useful in a self-contained breathing apparatus. 4KO2 + 2CO2 2K2CO3 + Oxygen for First Responders In self-contained breathing devices used by first responders, potassium superoxide, KO2, reacts with exhaled carbon dioxide to produce potassium carbonate and oxygen: 4 KO2(s) +2 CO2(g) 2 K9CO3(s) + 3 O2(g) How much O2 could be produced from 85 g KO2? It has the ionic structure (K +) (O2-). © 2013-2020 HomeworkLib - FREE homework help online, user contributions licensed under cc by-sa
social media Hence, it acts as limiting reagent. Well, remember, our number of moles is just mass divided by molecular weight. The scientific notation Another way we could, right? We could fix that if we put a three halves here and that would give us three and three is six Oxygen's on the right and for 56 on the left. But we started with a pretty small amount of stuff and now we're asked. A self-contained breathing apparatus uses potassium superoxide () reacting with carbon dioxide to produce potassium carbonate and oxygen. (12 pts.) ). So this time we need to divide by two and we end up with seven point zero three to times 10 to the minus six moules. (b) What is the rms speed of an O2 molecule at -9.4 oC? b) stick with headings and captions. How much O2 could be produced from 2.50 g of KO2 and 4.50 g CO2? Potassium superoxide $\left(\mathrm{KO}_{2}\right),$ a useful source of oxygen employed in breathing equipment, reacts with water to form potassium hydroxide, hydrogen peroxide, and oxygen. The models come up to the talk and we're left with and in bowls as we knew it should. 3O2. This is just say it's 1.0 kilograms because there are 1000 grams in a kilogram and that would be a more usual way to write it.
4.0, ANSWER: Molar Molar the mass of KO₂ = 71 g mass of co₂ = 44 g given equation - from 2 KO2 + co2 K₂CO3 +3,02 So, & un g co reacts with 2x71 g KO₂ 4.62 g co₂ reacts with 2x71 x 4.62 g 44 i e., 14.91 g KO₂ But only 2.45 g of ko, is available. K + O2(air) = KO2 (combustion, impurity K2O2). I have a 1993 penny it appears to be half copper half zink is this possible? Experiments indicate that 2 $\mathrm{mol}$ of $\mathrm{KO}_{2}(s)$ react with each mole of= $\mathrm{CO}_{2}(g) .$ (a) The products of the reaction are $\mathrm{K}_{2} \mathrm{CO}_{3}(s)$ and $\mathrm{O}_{2}(g) .$ Write a balanced equation for the reaction between $\mathrm{KO}_{2}(s)$ and $\mathrm{CO}_{2}(g) . 7.37. The superoxide consumes the $\mathrm{CO}_{2}$ exhaled by a person and replaces it with oxygen.$$4 \mathrm{KO}_{2}(\mathrm{s})+2 \mathrm{CO}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g})$$What mass of $\mathrm{KO}_{2}$, in grams, is required to react with $8.90 \mathrm{L}$ of $\mathrm{CO}_{2}$ at $22.0^{\circ} \mathrm{C}$ and $767 \mathrm{mm}$ Hg? of CO2? Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. Spell out the full name of the compound.? (\mathbf{b})$ Indicate the oxidation number for each atom involved in the reaction in part (a). So we need to again look at the stoke you metric coefficients for every full four moles of co two, we end up with two moles of potassium carbonate. How much O2 could …
Reacts with water, acids, mono-and carbon dioxide, ozone, potassium, ammonia. So for Ko to the molecular weight is going to be 39 poin 010 That's the atomic weight of that has waas twice oxygen, which is 16. It is a strong oxidizing agent. (2.50 g KO2) / (71.0972 g KO2/mol) = 0.0351631 mol KO2, (4.50 g CO2) / (44.0096 g CO2/mol) = 0.102250 mol CO2.
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