- #1

courtrigrad

- 1,236

- 2

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?