potassium superoxide. KO2 reacts with carbon dioxide, CO2 according to the following equations: 4 KO2 +...
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potassium superoxide. KO2 reacts with carbon dioxide, CO2 according to the following equations:
4 KO2 + 2 CO2 --> 2 K2CO3 + 3 O2
When 8 moles of KO2 and 3 moles of CO2 react, the limiting reagent and moles of O2 produced is:
KO2 limiting, 6.0 moles O2
CO2 limiting, 12.0 moles O2
KO2 limiting, 3.0 moles O2
CO2 limiting, 4.5 moles O2
Homework Answers
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potassium superoxide. KO2 reacts with carbon dioxide,
CO2 according to the following equations:
4 KO2 +...
Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and oxygen: 4KO2 + 2CO2...
Potassium superoxide, KO2, reacts with carbon dioxide
to form potassium carbonate and oxygen:
4KO2 + 2CO2 2K2CO3 +
3O2
This reaction makes potassium superoxide useful in a
self-contained breathing apparatus. How much O2 (in
grams) could be produced from 2.45 g of KO2 and 4.62 g
of CO2?
Potassium superoxide KO2 reacts with carbon dioxide to form potassium carbonate and oxygen 4KO2(s)+2CO2(g)-->2K2CO3(s)+3O2(g) How many...
Potassium superoxide KO2 reacts with carbon dioxide to form potassium carbonate and oxygen 4KO2(s)+2CO2(g)-->2K2CO3(s)+3O2(g) How many moles of O2 will be produced from 2.50 moles KO2 and 1.50 moles of CO2? Please show work using differential analysis
Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and...
Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. It is used in submarines, space vehicles, space suits, and by firefighters and miners. 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. (12 pts.) 7. When 12.424 g of (NH4),PO. (FW 149.087 g/mole) is...
Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. It reacts with carbon...
Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. It reacts with carbon dioxide and water in exhaled air to produce oxygen. 4KO2 + 2H2O + 4CO2 → 4KHCO3 + 302 If a person wearing such a mask exhales 0.702 grams of carbon dioxide per minute, how many grams of oxygen are produced in 5 minutes? Assume you have plenty of every other reagent. O 0.510 grams O 0.383 grams 1.91 grams 2.55 grams
The reaction between potassium superoxide, KO2, and CO2, 4KO2+2CO2→2K2CO3+3O2 is used as a source of O2...
The reaction between potassium superoxide, KO2, and CO2, 4KO2+2CO2→2K2CO3+3O2 is used as a source of O2 and absorber of CO2 in self-contained breathing equipment used by rescue workers. a). How many moles of O2 are produced when 0.475 mol of KO2 reacts in this fashion? b). How many grams of KO2 are needed to form 8.0 g of O2? c). How many grams of CO2 are used when 8.0 g of O2 are produced?
answer according to text book is 29 g of O2 produced from 85g , please show...
answer according to text book is 29 g of O2 produced from 85g
, please show all steps in how to solve!
7.37. 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?
A self-contained breathing apparatus uses canisters of potassium superoxide, KO2, which consumes the CO2 exhaled by...
A self-contained breathing apparatus uses canisters of potassium superoxide, KO2, which consumes the CO2 exhaled by a person and replaces it with oxygen according to the following reaction: 4KO2(s) + 2CO2(g) → 2K2CO3(s) + 3O2(g) (a) What mass of KO2 in g is required to convert 6.30 L of CO2 at 21.0 oC and 656 mmHg into O2? Answer _____________________ (b) What is the rms speed of an O2 molecule at -9.4 oC?
please provide all the steps 7.37. Oxygen for First Responders In self-contained breathing devices used by...
please provide all the steps
7.37. 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,?
Use the References to access important values if needed for this question. When carbon dioxide reacts...
Use the References to access important values if needed for this question. When carbon dioxide reacts with potassium hydroxide, potassium carbonate and water are produced. The balanced equation for this reaction is: CO2(g) + 2KOH(aq) + K,CO3(aq) + H2O(1) If 4 moles of carbon dioxide react, The reaction consumes The reaction produces moles of potassium hydroxide. moles of potassium carbonate and _moles of water
32. Aluminum hydroxide reacts with carbon dioxide as follows: 2 Al(OH)3 (aq) + 3 CO2 (g)...
32. Aluminum hydroxide reacts with carbon dioxide as follows: 2 Al(OH)3 (aq) + 3 CO2 (g) → Alz(CO3) (8) + 3 H20 Which is the limiting reactant when 3.0 mol Al(OH)3 and 4.0 mol CO2 are allowed to react? a) Al(OH)3 b) CO2 c) H20 d ) Alz(CO3)3 33. For the above reaction in problem 32, Which is the limiting reactant when 3.0 g of Al(OH)3 and 4.0 g of CO2 are allowed to react? a) Al(OH)3 b) CO2 c)...
Potassium superoxide, KO2, reacts with carbon dioxide
to form potassium carbonate and oxygen:
4KO2 + 2CO2 2K2CO3 +
3O2
This reaction makes potassium superoxide useful in a
self-contained breathing apparatus. How much O2 (in
grams) could be produced from 2.45 g of KO2 and 4.62 g
of CO2?
Potassium superoxide (KO2) reacts with carbon dioxide to produce oxygen in reaction is very fast and nearly quantitative. It is used in submarines, space vehicles, space suits, and by firefighters and miners. 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. (12 pts.) 7. When 12.424 g of (NH4),PO. (FW 149.087 g/mole) is...
Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. It reacts with carbon dioxide and water in exhaled air to produce oxygen. 4KO2 + 2H2O + 4CO2 → 4KHCO3 + 302 If a person wearing such a mask exhales 0.702 grams of carbon dioxide per minute, how many grams of oxygen are produced in 5 minutes? Assume you have plenty of every other reagent. O 0.510 grams O 0.383 grams 1.91 grams 2.55 grams
answer according to text book is 29 g of O2 produced from 85g
, please show all steps in how to solve!
7.37. 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?
please provide all the steps
7.37. 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,?
Use the References to access important values if needed for this question. When carbon dioxide reacts with potassium hydroxide, potassium carbonate and water are produced. The balanced equation for this reaction is: CO2(g) + 2KOH(aq) + K,CO3(aq) + H2O(1) If 4 moles of carbon dioxide react, The reaction consumes The reaction produces moles of potassium hydroxide. moles of potassium carbonate and _moles of water
32. Aluminum hydroxide reacts with carbon dioxide as follows: 2 Al(OH)3 (aq) + 3 CO2 (g) → Alz(CO3) (8) + 3 H20 Which is the limiting reactant when 3.0 mol Al(OH)3 and 4.0 mol CO2 are allowed to react? a) Al(OH)3 b) CO2 c) H20 d ) Alz(CO3)3 33. For the above reaction in problem 32, Which is the limiting reactant when 3.0 g of Al(OH)3 and 4.0 g of CO2 are allowed to react? a) Al(OH)3 b) CO2 c)...
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