• half
• half
• one
• two

• k[H₂] [NO]²
• k[H₂O₂]²
• k[N₂][H₂O₂]²
• k[H₂O₂] [H₂]

• Temperature
• Mass
• Weight
• Time

• Increases as the reaction proceeds
• Decreases as the reaction proceeds
• May increase or decrease during the reaction
• Remains constant as the reaction proceeds

• Whose rate is affected by concentration.
• In which concentration of the reactants does not change with time.
• In which reactants do not react.
• In which one of the reactants is in large excess.

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

• 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

238. What will be the order of reaction if doubling of the concentration of a reactant increases the rate by a factor of 4 and trebling the concentration of the reactant by factor of 9?

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

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

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