Question

9) The equation for the reaction between potassium superoxide and carbon dioxide is given below: 4...

9) The equation for the reaction between potassium superoxide and carbon dioxide is given below:
4 KO2 + 2 CO2 ® 2 K2CO3 + 3 O2
How many grams of oxygen can be produced by the reaction of 25.00 g of KO2 and 11.00 g of CO2? (8)
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

4 KO2 +   2 CO2   -------------> 2 K2CO3 + 3 O2

284.4 g      88.02 g                      276.411 g    96 g

25.00 g      11.00 g

284.4 g KO2 --------------> 88.02 g CO2

25.0 g KO2 ---------------->    ??

mass of CO2 needed = 25.00 x 88.02 / 284.4

                                  = 7.737 g

so CO2 is excess .

here limiting reagent is KO2

284.4 g KO2 --------------> 96 g O2

25.0 g KO2 ---------------->    ??

mass of CO2 produced = 25.0 x 96 / 284.4

                                     = 8.439 g

mass of CO2 produced = 8.439 g

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Potassium superoxide, KO2, reacts with carbon dioxide to form potassium carbonate and dioxygen as follows: 4KO2+...
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?
The reaction of potassium superoxide, KO2, is used in life-support systems to replace CO2(g) in expired...
The reaction of potassium superoxide, KO2, is used in life-support systems to replace CO2(g) in expired air with O2(g). 4KO2(s)+2CO2(g)→2K2CO3(s)+3O2(g) a) How many moles of O2(g) are produced by the reaction of 100 g CO2(g) with excess KO2(s)? b) How many grams of KO2(s) are consumed per 1000.0 g CO2(g) removed from expired air? c) How many moles K2CO3 are produced per milligram of KO2 consumed?
Problem 3.62 The reaction between potassium superoxide, KO2, and CO2, 4KO2+2CO2→2K2CO3+3O2 is used as a source...
Problem 3.62 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. (Figure 1) Part A How many moles of O2 are produced when 0.350 mol of KO2 reacts in this fashion? Express your answer with the appropriate units. n(O2) = 0.263 mol SubmitMy AnswersGive Up Correct Part B How many grams of KO2 are needed to form 6.0 g of O2?...
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon...
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon dioxide and iron metal is given below. Fe2O3 (s) + 3 CO (g) --> 2 Fe (s) + 3 CO2 (g) Using the balanced equation, determine the mass of iron metal (Fe(s)) in grams that can be made if this reaction is performed using 225.3 grams of iron (III) oxide (Fe2O3) and 200.1 grams of carbon monoxide.
How many grams of carbon dioxide are formed if 0.164 moles of ethanol (CH3CH2OH) react with...
How many grams of carbon dioxide are formed if 0.164 moles of ethanol (CH3CH2OH) react with 80 grams of oxygen according to the following balanced equation: CH3CH2OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l)
Consider the neutralization reaction between potassium carbonate, K2CO3, and hydrobromic acid, HBr, forming the salt potassium...
Consider the neutralization reaction between potassium carbonate, K2CO3, and hydrobromic acid, HBr, forming the salt potassium bromide, KBr, carbon dioxide, CO2, and water, H2O. The balanced chemical equation for the reaction is K2CO3(aq)+2HBr(aq)→2KBr(aq)+CO2(g)+H2O(l) In the reaction, K2CO3, HBr, and KBr are strong electrolytes, so these compounds dissociate completely in water to form their respective ions. The total ionic equation is 2K+(aq) + CO32−(aq) + 2H+(aq) + 2Br−(aq)→2K+(aq) + 2Br−(aq) + CO2(g) + H2O(l) To obtain the net ionic equation, the...
32. Refer to the following unbalanced equation: C6H14 + O2 ® CO2 + H2O What mass...
32. Refer to the following unbalanced equation: C6H14 + O2 ® CO2 + H2O What mass of carbon dioxide (CO2) can be produced from 11.2 g of C6H14 and excess oxygen?
Pentane gas, C5H12 undergoes combustion with oxygen gas to produce carbon dioxide and water gases. a....
Pentane gas, C5H12 undergoes combustion with oxygen gas to produce carbon dioxide and water gases. a. Write the balanced chemical equation. b. How many grams of C5H12 are needed to produce 72 g of water? c. How many grams of CO2 are produced from 32.0 g of O2" please type and explain how you got the answer
In the following chemical reaction, how many moles of O2 are needed to produce 2.8 mol...
In the following chemical reaction, how many moles of O2 are needed to produce 2.8 mol of CO2? C2H6 + O2 → CO2 + H2O? How many moles of methane are produced when 36.6 moles of carbon dioxide gas react with excess hydrogen gas? How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 53.6 moles of water vapor? Plants convert carbon dioxide and water to glucose (C6H12O6) and oxygen in the process...
Gaseous ethane CH3CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and...
Gaseous ethane CH3CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 0.30 g of ethane is mixed with 2.20 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT