Question
Challenge Nitrogen and oxygen gases react to form dinitrogen oxide gas $\left(\mathrm{N}_{2} \mathrm{O}\right) .$ What volume of $\mathrm{O}_{2}$ is needed to produce 34 L of $\mathrm{N}_{2} \mathrm{O}$ ?
Step 1
However, the equation is not balanced. The unbalanced equation is: \[N_2 + O_2 \rightarrow N_2O\] Show more…
Show all steps
Your feedback will help us improve your experience
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. $$ 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{NO}_{2}(\mathrm{g}) $$ (a) You wish to react $\mathrm{NO}$ and $\mathrm{O}_{2}$ in the correct stoichiometric ratio. The sample of NO has a volume of 150 mL. What volume of $\mathrm{O}_{2}$ is required (at the same pressure and temperature)? (b) What volume of $\mathrm{NO}_{2}$ (at the same pressure and temperature) is formed in this reaction?
Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. $$2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{g})$$ (a) If you mix $\mathrm{NO}$ and $\mathrm{O}_{2}$ in the correct stoichiometric ratio, and NO has a volume of $150 \mathrm{mL}$, what volume of O, is required (at the same pressure and temperature)? (b) After reaction is complete between 150 mL of $\mathrm{NO}$ and the stoichiometric volume of $\mathrm{O}_{2},$ what is the volume of $\mathrm{NO}_{2}$ (at the same pressure and temperature)?
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD