Given the following balanced reaction between nitrogen gas and oxygen gas to produce nitrous oxide gas, how many moles of nitrous oxide gas are produced from 1.65 moles of nitrogen gas?

Question

anonymous · Answer

For the first part that is to give the balanced chemical reaction, make a rough sketch of the reaction first : 

$N_2 (g) + O_2 (g) \rightarrow N_2 O (g) $ 

Now balance it.

anonymous · Answer

For the second part, $\textbf{It is important for us to assume that there is no excess of oxygen.}$ 

Thus, in the balanced chemical equation, you'll realize that 2 moles of $N_2$ is on LHS while 2 moles of $N_2 O$ is on RHS. So , 1 moles of $N_2$ will produce 1 mole of $N_2 O$ . Thus, 1.65 moles of $N_2$ will produce 1.65 moles of $N_2 O$ 


$\large{\mathsf{Note :}} \
 \large{\space \bullet \space \textbf{This is a combustion reaction.} \
 \space \bullet \textbf{ If there was excess of oxygen then the product would  } \
\space \space \space \space \space \textbf{have been changed to other nitrogen oxides. }} $