Question

Which of the following is the balanced reaction, given the rate relationships below.

a. rate = − 13   Δ[CH4] Δt = − 12   Δ[H2O] Δt = − Δ[CO2] Δt = 14   Δ[CH3OH] Δt
b. rate = − 12   Δ[N2O5] Δt = 12   Δ[N2] Δt = 15   Δ[O2] Δt
c. rate = − 12   Δ[H2] Δt = − 12   Δ[CO2] Δt = − Δ[O2] Δt = 12   Δ[H2CO3] Δt

Answer 1

a.
`3CH_4+2H_2O+CO_2\rightarrow 4CH_3OH`

b.
`2N_2O_5\rightarrow 2N_2 + 5O_2`

c.
`2H_2+2CO_2+O_2\rightarrow 2H_2CO_3`

Step-by-step explanation:

Hello,

In this case, since those rate relationships have the stoichiometric coefficient at the denominators of the fractions preceding each ratio and the negative terms account for reactants and positive for products, we have:

a.
`3CH_4+2H_2O+CO_2\rightarrow 4CH_3OH`

b.
`2N_2O_5\rightarrow 2N_2 + 5O_2`

c.
`2H_2+2CO_2+O_2\rightarrow 2H_2CO_3`

Best regards.