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OpenStudy (anonymous):
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.
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OpenStudy (jfraser):
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 \(8H_2S + 4O_2\)
OpenStudy (jfraser):
the products follow the same rules
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