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. So C n is mass divided by molecular weight says what we want to do right now. And the question is how much oxygen and I were going to produce.

4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g) That's the same as 1.0 times 10 to the minus three grands, Or if you write that not in scientific notation.

Then the potassium hydroxide reacts with carbon dioxide to produce potassium carbonate. Potassium superoxide is the inorganic compound with the formula KO 2. Okay, and now t work out the Mass. Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen:? 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.

And that gives us exactly to a point 00 moles of co two that we consume. And here I like to show the units because now we're reassuringly the grandes cancel. Potassium superoxide due to chemical reaction with respiratory exhaustion gases including steam and CO 2 gas, while gradually producing O 2 gas eliminates CO 2 gas because potassium superoxide is one of the most efficient and practical methods of carbon dioxide absorption and its exact quotient respiratory system (SRQ). The first thing we need to do is calculate the molecular weeds for later in the problem. Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen: 4KO2 + 2CO2 ----> 2K2CO3+3O2. So we need to again look at the stoke you metric coefficients. 7.37.

It produces potassium carbonate and oxygen. Do radioactive elements cause water to heat up? 7.37. eval(ez_write_tag([[468,60],'homeworklib_com-large-leaderboard-2','ezslot_12',136,'0','0'])); 7.37. It is used in submarines, space vehicles, space suits, and by firefighters and miners. Now that we have a balanced reaction, we could do some calculations and we're told that we have 88 grams of carbon dioxide in the presence of excess potassium super oxide. And this time I've included the coefficients for the balance equal usually work those Odin party. The unbalanced chemical equation for the reaction is given below.$\mathrm{Al}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{s}) \longrightarrow$$$\mathrm{Al}_{2}^{4} \mathrm{O}_{3}(\mathrm{s})+\mathrm{AlCl}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{N}_{2}(\mathrm{g})$$What is the minimum mass of $\mathrm{NH}_{4} \mathrm{ClO}_{4}$ consumed, per kilogram of $\mathrm{Al},$ by the reaction of $\mathrm{NH}_{4} \mathrm{ClO}_{4}$ and Al? So that's going to be our 1.0 times 10 to the minus three grounds divided by the 71.1 grams per mole. answer according to text book is 29 g of O2 produced from 85g 24 grams of magnesium metal reacts with 16 grams of oxygen gas to form magnesium oxide according to the law of conservation of mass how much magnesium oxide will there be after the chemical change is complete.

A self-contained breathing apparatus uses potassium superoxide () reacting with carbon dioxide to produce potassium carbonate and oxygen. That's a reaction. 4KO2 ​+ 2CO2 ​ 2K2CO3 + It reacts with carbon dioxide and water in exhaled air to produce oxygen. 4KO2 + 3C (graphite) = 2K2CO3 + CO2 (30°C).

Potassium superoxide, KO2, is used for producing oxygen and removing carbon dioxide in selfcontained breathing units, space shuttles, and other enclosed spaces. Potassium Superoxide ($\ce{KO2}$) is used as an oxygen provider and carbon dioxide scrubber in life support systems $$\ce{2KO2 + H2O -> 2KOH + O2} \\ \ce{2KOH + CO2 -> K2CO3 + H2O}$$ I encountered a question that asked if Potassium superoxide can also serve as a scrubber for $\ce{CO}$. Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. Potassium superoxide, KO2, reacts with carbon dioxide Oxygen for First Responders In self-contained breathing devices used by first responders, potassium superoxide, $\mathrm{KO}_{2}$ reacts with exhaled carbon dioxide to produce potassium carbonate and oxygen:$$4 \mathrm{KO}_{2}(s)+2 \mathrm{CO}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(s)+3 \mathrm{O}_{2}(g)$$How much $\mathrm{O}_{2}$ could be produced from $85 \mathrm{g} \mathrm{KO}_{2} ?$, 5. Spell out the full name of the compound.. Here we have four and two is six, and over here we have three and we don't have six year. Please explain step by step, thank you! True False. Potassium superoxide, KO 2, reacts with carbon dioxide to form potassium carbonate and oxygen: 4KO 2 + 2CO 2 2K 2 CO 3 + 3O 2 . This was very easy, but another way we could get that if that wasn't exactly two, is we just take the moles of oxygen and we multiply it by three after divided by two.

That's 32 okay, and those are all in grams per mole. It gives us a lot of grands, so we could write it as 3000 200 and 31 grams. Some rebreathers use lithium hydroxide canisters. What elements are being oxidized and reduced? Governor issues overnight stay-at-home advisory, Battle intensifies over which votes will count, The 12 states that will determine the 2020 election, For a closing argument, Trump attacks LeBron, Stern commends Swift for taking a political stance, Betting markets see Trump losing as battlegrounds shift, Report: Soccer legend Diego Maradona hospitalized, Fox ratchets up parenting spat with estranged husband, Alert: Hand sanitizer could disqualify your ballot, 'Not backing down': Amazon workers want time to vote, LeBron James endorses Biden after Trump attack. Assume you have plenty of every other reagent. T... üven 50 CO 3 oul At uods A 50 50 A Nods B 100 106 NOW 950... cal intersection is line Cary, z) = (215,2)= (215,0) + (0... 16.The shaft of the long bone - diaphysis. O 0.510 grams O 0.383 grams 1.91 grams 2.55 grams. 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 KO,(s) + 2 CO2(g) – 2 K2CO3(s) + 3 O2(g) How much O, could be produced from 85 g KO,? (a) Write equations for these two reactions and comment on the effectiveness of potassium superoxide in this application. Potassium superoxide react with carbon dioxide to produce potassium carbonate and oxygen. Therefore, it is used as the preferred chemical oxygen supply in under-mine refuge chambers. eval(ez_write_tag([[250,250],'homeworklib_com-leader-1','ezslot_13',111,'0','0'])); Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen:? Need help with 1-3 Assume that $\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s})$ is the only source of $\mathrm{O}_{2}(\mathrm{g}) .$ [Hint: Write a balanced equation for the reaction.]. 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. of CO2? first calculate the number of moles of CO2 (R=0.08026 L*atoms/ mol*K)find moles of Co2 and mass of KO2 in grams? But we are keeping track, and for CO. Two is going to be wells 0.1 and two times 16. Get your answers by asking now. (c) How many liters of respired air can react with $7.00 \mathrm{g}$ of $\mathrm{KO}_{2}$ if each liter of respired air contains $0.063 \mathrm{g}$ of $\mathrm{CO}_{2} ?$, Potassium superoxide, $\mathrm{KO}_{2},$ reacts with carbon dioxide to form potassium carbonate and oxygen:$4 \mathrm{KO}_{2}(s)+2 \mathrm{CO}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(s)+3 \mathrm{O}_{2}(g)$.This reaction makes potassium superoxide useful in a self-contained breathing apparatus. social media Potassium superoxide is sensitive to moisture in the air. How much O2 could be produced from 2.50 g of KO2 and 4.50 g CO2? I have a 1993 penny it appears to be half copper half zink is this possible? And that's just three points.

b) stick with headings and captions. © 2013-2020 HomeworkLib - FREE homework help online, user contributions licensed under cc by-sa 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. Still have questions? 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? could i have help for the answers for the molecular eq, ionic eq, net ionic eq and spectator ions or these reactions? Answer _____________________ We really just need to co two at the oxygen, but we're going to need them all for the rest of the problem anyway, So let's go ahead and calculate them.

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. How much O2 could be produced from 2.50 g of KO2 and 4.50 g CO2? What is the mass percent $\mathrm{Fe}_{2} \mathrm{O}_{3}$ in the ore sample, assuming that none of the impurities contain Fe? Please kindly go through the attached question below, and help If the oxygen supply becomes limited or if the air becomes poisoned, a worker can use the apparatus to breath. the CO2 exhaled by... A self-contained breathing apparatus uses potassium superoxide () reacting with carbon dioxide to produce potassium carbonate and oxygen. How much O2 could … Join Yahoo Answers and get 100 points today. And if we wanted to write that in milligrams, that would becomes zero point 97 19 because there are 1000 milligrams in a grand, so the number is going to get 1000 times bigger, Rita.

self-contained breathing apparatus. Potassium superoxide is a strong oxidant, able to convert oxides into peroxides or molecular oxygen. What is the correct name for the compound CaSO4. So that gives us 96.0. 2KO2 + H2SO4 (anhydrous) = K2SO4 + O3↑ + H2O (normal temp.). 4KO2 + 2CO2 (humidity) = 2 K2CO3 + 3O2 (normal temp.). It is a rare example of a stable salt of the superoxide anion. 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. 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.

, please show all steps in how to solve! Or for bulls times the molecular weight 71.1 And that's in grams per mole and happily are moles. How Much O2 Could Be Produced From 2.45g Of KO2 And 4.60 G Of CO2? 7. (a) Write an equation for the reaction. You must be logged in to bookmark a video. How much O 2 (in grams) could be produced from … We mean that it means we know the reaction will continue until all this CO two is consumed. Click 'Join' if it's correct. So that's going to be our 1000 grams divided by 44.1 grams per mole, and that gives us 22 0.72 molds. How much $\mathrm{O}_{2}$ could be produced from $2.50 \mathrm{g}$ of $\mathrm{KO}_{2}$ and $4.50 \mathrm{g}$ of $\mathrm{CO}_{2} ?$. profile pages. Chemical reactions with potassium superoxide KO2: KO2 -O2→(290°C, vacuum) K2O2 -O2 → (530°C) K2O. And now we're told, What if we have one times 10 to the three grams of CO two. 4KO2(s) + 2H2O(l) --> 4KOH(s) + 3O2(g) The figure shows an initially stationary block of mass ! grams) could be produced from 2.45 g of KO2 and 4.62 g (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. So for the next part, remember I said we were going to need the molecular weights. And we wanted to know in this case how much Seo too, did we also consume. We know we wanted a number Ingram's and that gives us.

Well, remember, our number of moles is just mass divided by molecular weight. superoxide, KO2, which consumes So now we can calculate our number of moles of CO two and number of moles is just mass over molecular weight.



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