Write a balanced reaction for which the following rate relationships are true. Rate = -1/2 * Delta[N2O5]/Delta T = 1/4 * Delta[NO2]/Delta T = Delta[O2]/ Delta T

Question

A. 1/4 NO₂ + O₂  →  _1/2 N₂O₅ 

B. 4 NO₂ + O₂  →  2 N₂O₅

_C. 2 N₂O₅ → NO₂ + 4 O₂

_D. 2 N₂O₅ → 4 NO₂ + O₂

_{E. 1/2} N₂O_{5 →  1/4} NO₂ + O₂

Answer 1

The -1/2 ∆N₂O₅/∆t tells us that N₂O₅ is a reactant since it is disappearing (hence the minus sign). It also tells us that the coefficient is 2 (hence the 1/2). So, we know the reactant is 2N₂O₅.

The +1/4 ∆NO₂/∆t tells us the NO₂ is a product because it is appearing (hence the plus sign). It also tells us that the coefficient is 4 (hence the 1/4). So, we know the product is 4NO₂.

The +∆O₂/∆t tells us the O₂ is a product because it is appearing (hence the positive value). It also tells us the the coefficient is 1, so we know the product is O₂.

With this information, we can write the balanced equation as...

2N₂O₅ ==> 4NO₂+ O₂