Consider the reaction:
8H2S(g)+4O2(g)→8H2O(g)+S8(g)
Δ[H2S]/Δt = -0.033M/s .

Find Δ[O2]/Δt
Δ[H2O]/Δt
Δ[S8]/Δt
Find the rate of the reaction.

Question

Consider the reaction:
8H2S(g)+4O2(g)→8H2O(g)+S8(g)
Δ[H2S]/Δt = -0.033M/s .

Find Δ[O2]/Δt
Δ[H2O]/Δt
Δ[S8]/Δt
Find the rate of the reaction.

jfraser · Answer

the changes in concentrations follow the same patterns as the coefficients in the balanced reaction.

If the hydrogen sulfide is changing at 4M/s, then the oxygen must be changing at $half$ that rate, because the coefficients are $8H_2S + 4O_2$

jfraser · Answer

the products follow the same rules