The depletion of ozone (O_3) in the stratosphere has been a matter of great conc
ID: 535955 • Letter: T
Question
The depletion of ozone (O_3) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitric oxide (NO) that is discharged from high- altitude jet planes. The reaction is: O_3 + NO rightarrow O_2 + NO_2 If 0.740 g of o3 reacts with 0.703 g of NO, how many grams of NO_2 will be produced? Which compound is the limiting reactant? Calculate the number of moles of the excess reactant remaining at the end of the reaction. How many grams of NO_2 will be produced? Which compound is the limiting reactant? O_3 NO How many moles of the excess reactants remain at the end of the reaction? molExplanation / Answer
One mole of ozone reacts with one mole of nitric oxide to give one mole of oxygen gas and one mole of nitrogen dioxide.
Molecular mass of O3 = 48g
Molecular mass of NO = 30g
Molecular mass of NO2 = 46g
0.740g of O3 is 0.0154167 moles
0.703g of NO is 0.023433 moles
So, 0.0145167 moles of NO2 is produced which is 0.709167g.
The limiting reagent is O3. 0.0080163 moles of NO remains unreacted at the end of reaction.