How many moles of [tex]$O_2$[/tex] gas react with 2 moles of NO gas according to the following balanced chemical equation?
[tex]2 NO(g)+O_2(g) \longrightarrow 2 NO_2(g)[/tex]
A. [tex]$2 mol O_2$[/tex]
B. [tex]$4 mol O_2$[/tex]
C. [tex]$1 mol O_2$[/tex]
D. [tex]$0.5 mol O_2$[/tex]
E. none of the above
Answer (1)
The balanced chemical equation 2 NO ( g ) + O 2 ( g ) → 2 N O 2 ( g ) indicates that 2 moles of NO react with 1 mole of O 2 .
Determine the mole ratio between NO and O 2 from the balanced equation, which is 2:1.
Calculate the moles of O 2 required to react with 2 moles of NO using the mole ratio: 2 1 × 2 = 1 .
Therefore, 1 mole of O 2 is needed to react with 2 moles of NO , so the answer is 1 m o l O 2 .
Explanation
Analyze the balanced equation We are given the balanced chemical equation: 2 NO ( g ) + O 2 ( g ) → 2 N O 2 ( g ) . This equation tells us that 2 moles of NO gas react with 1 mole of O 2 gas to produce 2 moles of N O 2 gas. We are asked to find out how many moles of O 2 react with 2 moles of NO.
Determine the mole ratio From the balanced equation, we can see that the ratio of moles of NO to moles of O 2 is 2:1. This means that for every 2 moles of NO, we need 1 mole of O 2 .
Calculate moles of Oxygen Since we have 2 moles of NO, we can use the mole ratio to find the moles of O 2 needed: moles of NO moles of O 2 = 2 1 moles of O 2 = 2 1 × moles of NO moles of O 2 = 2 1 × 2 = 1 Therefore, 1 mole of O 2 is required to react with 2 moles of NO.
Examples
In the Haber-Bosch process, nitrogen and hydrogen react to form ammonia. Understanding stoichiometry, like in this problem, is crucial for optimizing the production of ammonia, ensuring the correct ratio of reactants to maximize yield and minimize waste. This principle applies to many industrial chemical processes where precise control of reactant quantities is essential for efficiency and cost-effectiveness.
