43.2k views
3 votes
How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

User Coldfix
by
7.6k points

2 Answers

6 votes
Hope this helps you!
How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to-example-1
User MaiOM
by
8.0k points
1 vote

Answer:0.28975 moles of nitrogen are formed .

Step-by-step explanation:


4KNO_3(s)\rightarrow 2K_2O(s)+2N_2(g)+5O_2(g)

Number of moles of
KNO_3=\frac{\text{Mass of the}KNO_3}{\text{Molar mass of the}KNO_3}=(58.6 g)/(101.11 g/mol)=0.5795 moles

According to reaction , 4 mol of
KNO_3 produces 2 moles of
N_2 gas.

Then,0.5795 moles of
KNO_3 will produce=
(2)/(4)* 0.5795 moles of
N_2 gas:


(2)/(4)* 0.5795=0.28975 moles

0.28975 moles of nitrogen are formed.

User Noah Stahl
by
8.3k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.