Question

Chemical Equations

Instructions: Solve the following chemical equations.

For the following reaction, calculate how many moles of NO2forms when 0.356 moles of the reactant completely reacts. 2 N2O5(g) ---> 4 NO2(g) + 02(g)

Answer 1

0.712 moles of NO₂ are formed.

Step-by-step explanation:

First, we need to write the balanced equation:

2 N₂O₅(g) ⇄ 4 NO₂(g) + O₂(g)

From the balanced equation, we can see the relationship between the moles of N₂O₅ and the moles of NO₂. Every 2 moles of N₂O₅ that react, 4 moles of NO₂ are formed. Let us apply this relationship to the information given by the problem (0.356 moles of N₂O₅):

`0.356molN_(2)O_(5).(4molNO_(2))/(2molN_(2)O_(5)) =0.712molNO_(2)`