Solution Found!
Potassium nitrate decomposes on heating, producing
Chapter 3, Problem 42P(choose chapter or problem)
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen:
\(4 \mathrm{KNO}_{3}(\mathrm{~s}) \rightarrow 2 \mathrm{~K}_{2} \mathrm{O}(\mathrm{s})+2 \mathrm{~N}_{2}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g})\)
To produce \(56.6 kg\) of oxygen, how many
Moles of \(\mathrm{KNO}_{3}\) must be heated?
Grams of \(\mathrm{KNO}_{3}\) must be heated?
Equation Transcription:
4KNO3(s) 2K2O(s) + 2N2(g) + 5O2(g)
KNO3
Text Transcription:
4KNO_3(s) rightarrow 2K_2O(s) + 2N_2(g) + 5O_2(g)
56.6 kg
KNO_3
Questions & Answers
QUESTION:
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen:
\(4 \mathrm{KNO}_{3}(\mathrm{~s}) \rightarrow 2 \mathrm{~K}_{2} \mathrm{O}(\mathrm{s})+2 \mathrm{~N}_{2}(\mathrm{~g})+5 \mathrm{O}_{2}(\mathrm{~g})\)
To produce \(56.6 kg\) of oxygen, how many
Moles of \(\mathrm{KNO}_{3}\) must be heated?
Grams of \(\mathrm{KNO}_{3}\) must be heated?
Equation Transcription:
4KNO3(s) 2K2O(s) + 2N2(g) + 5O2(g)
KNO3
Text Transcription:
4KNO_3(s) rightarrow 2K_2O(s) + 2N_2(g) + 5O_2(g)
56.6 kg
KNO_3
ANSWER:
Step 1 of 2
Here we will have to find out amount of heated in moles and gram to form 56.6 kg of oxygen.
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen:
(a)
Moles of heated to produce 56.6 kg of oxygen
Given:
Mass of Oxygen = 56.6 kg = 56600 gram
Here 5 mole of has formed from 4 moles of
.
Molar mass of oxygen = 32.00 g/mole
We can use the conversion factor =
The mole of heated can be calculated as,
Thus 
is heated to produce 56.6 kg of oxygen.
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