Answer:
<em>The limiting reactant is </em><u><em>Carbon dioxide, </em></u>![CO_{2}](https://tex.z-dn.net/?f=CO_%7B2%7D)
Explanation:
The balanced reaction equation is:
→ ![CH_{4} N_{2} O + H_{2} O](https://tex.z-dn.net/?f=CH_%7B4%7D%20N_%7B2%7D%20O%20%2B%20H_%7B2%7D%20O)
The mole ratio of ammonia to carbon dioxide is 2:1
142100/17g = 8358.8 mol of NH3
211400/44g = 4, 804.5 mole of CO2
Now:
4,804.5 mol of CO2 ×
= 9,609 mol of NH3 present
8,358.8 mole of NH3 ×
= 4,179.4 mol of CO2 present
<em>NH3 needs 8, 358.8 moles but had 9, 609 moles⇒ excess reactant</em>
<em>CO2 needs 4, 804,5 mol but had 4, 179.4 moles⇒ limiting reactant (used up completely)</em>
<u>The limiting reactant is carbon dioxide, CO2.</u>