1.How would temperature effect the rate of a reaction? Would it increase its kinetic energy thereby speeding up the reaction. Is it right in saying that as the temperature increases, the frequency of collisions increases between molecules, and the orientation changes?(adsbygoogle = window.adsbygoogle || []).push({});

2. If we have [tex] 4Fe + 3O_{2} \rightarrow 2Fe_{2}O_{3} [/tex] and we know that the concentration of [tex] O_{2} [/tex] changes 0.05 mol/L every 2 seconds what is the rate of disappearance of [tex] Fe [/tex] in [tex] mol/L*sec [/tex]? So [tex] -\frac{1}{4} \frac{\Delta[Fe]}{\Delta t} = -\frac{1}{3} \frac{\Delta[O_{2}]}{\Delta t} = \frac{1}{2} \frac{\Delta[Fe_{2}O_{3}]}{\Delta t} [/tex]. In one second the rate of disappearance of [tex] O_[2} [/tex] would be 0.025 mol/L. So would it be [tex] \frac{0.025}{3} [/tex] for the rate of disappearance of [tex] Fe [/tex]? For the rate of evolution of [tex] Fe_{2}O_{3} [/tex] would be [tex] 2 \times 0.025 [/tex]?

3. If we have a reaction between X and Z and the rate law is [tex] k[X]^{2}[Z]^{3} [/tex] what would happen if:

a. concentration of X doubled while Z remains constant

b. concentration of Z triples while X remains constant

c. concentrations of both X and Z are doubled

For (a) would the rate quadruple because X has a reaction order of 2? For (b) would the rate go up by a factor of 8? For (c) would the rate go up by a factor of 16?

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# Homework Help: Properties of Reactions

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