Recall that for a reaction **aA ****→**** bB**, the ** rate of a reaction** is given by:

$\overline{){\mathbf{Rate}}{\mathbf{=}}{\mathbf{-}}\frac{\mathbf{1}}{\mathbf{a}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{A}\mathbf{\right]}}{\mathbf{\Delta t}}{\mathbf{=}}\frac{\mathbf{1}}{\mathbf{b}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{B}\mathbf{\right]}}{\mathbf{\Delta t}}}$

where:

**Δ[A]** = change in concentration of reactants or products (in mol/L or M), *[A] _{final} – [A]_{initial}*

**Δt** = change in time, *t _{final} – t_{initial}*

**Reaction: 3 O _{2} + 2 CH_{3}OH → 2 CO_{2} + 4 H_{2}O**

H_{2}O is a product, the rate with respect to H_{2}O is *positive (+)* since we’re *gaining products*.

O_{2} is a reactant, the rate with respect to O_{2} is *negative (–)* since we’re *losing reactants*.

Given the following balanced chemical equation

3 O_{2} + 2 CH_{3}OH → 2 CO_{2} + 4 H_{2}O

How is the rate of appearance of H_{2}O related to the rate of disappearance of O_{2}?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Average Rate of Reaction concept. You can view video lessons to learn Average Rate of Reaction. Or if you need more Average Rate of Reaction practice, you can also practice Average Rate of Reaction practice problems.