IN ORDER TO RECEIVE FULL MARKS, SHOW ALL OF YOUR WORK AND PROVIDE FULL JUSTIFICA
ID: 848124 • Letter: I
Question
IN ORDER TO RECEIVE FULL MARKS, SHOW ALL OF YOUR WORK AND PROVIDE FULL JUSTIFICATION FOR ANY CONCLUSIONS YOU MAKE. PLEASE BE NEAT. CLEARLY SHOW THE ANSWERS FOR EACH OF THE THREE QUESTIONS BELOW. IF YOU USE MORE THAN ONE SHEET OF PAPER. SIGN ALLTHE SHEETS AN STAPLE THEM TOGETHER. DO YOUR ROUGH WORK ELSEWHERE,THEN COPY YOUR NEAT WORK ONTO THIS PAGE. MESSY AND DISORGANIZED WORK WILL NOT BE GRADED. The depletion of ozone (O,) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitrogen monoxide that is discharged from high altitude jet planes. The reaction is: O3(g) + NO(g) rightarrow02(g)+NO2(g) If 1.740 g of ozone reacts with 1.670 g of nitrogen monoxide, which compound is the limiting reactant ? how many grams of nitrogen dioxide will be produced? what is the mass of the excess reactant remaining at the end of the reaction ?Explanation / Answer
a) moles of O3 = 1.74/48 = 0.036 moles
moles of NO = 1.67/30 = 0.056 moles
so limitnig reagent is O3 s its moles is less
b) moles of NO2 produced = 0.036 moles
so mass of NO2 =1.656g
c) moles of NO remaining at the end of reaction = 0.056-0.036 = 0.02 moles
so mass of NO remaning = 0.02*30 = 0.6g
explained in details