For the reaction $\mathrm{aA}+\mathrm{bB}\to \mathrm{mM}+\mathrm{nN}\frac{-\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}$ is equal to

• $\frac{-\mathrm{d}\left[\mathrm{B}\right]}{\mathrm{dt}}$
• $\frac{\mathrm{a}}{\mathrm{m}}-\frac{\mathrm{d}\left[\mathrm{M}\right]}{\mathrm{dt}}$
• $\frac{-\mathrm{b}}{\mathrm{a}}\frac{-\mathrm{d}\left[\mathrm{B}\right]}{\mathrm{dt}}$
• $-\frac{1}{\mathrm{b}}\frac{\mathrm{d}\left[\mathrm{B}\right]}{\mathrm{dt}}$

For the reaction A B, the rate of reaction becomes twenty seven times when the concentration of A is increased three times.
What is the order of the reaction?

• first order
• zero order
• second order
• third order

• A chemical reaction occurs with every molecular collision
• Rate is directly proportional to the number of collisions per second
• Reactions in the gas phase are always of zero order
• Reaction rates are of the order of molecuar speeds

• k = 10²
• k = 10^–2
• k = 10
• k = 1