REACTION KINETICS

Given the following balanced equation :

2NO(g) + Cl₂(g) → 2NOCl(g)

If the rate of disappearance of Cl₂ is 4.84 x 10^-2 Ms^-1, what is the rate of disappearance of NO?

• 1.45 x 10^-2 Ms^-1

• 2.42 x 10^-2 Ms^-1

• 3.67 x 10^-2 Ms^-1

• 9.68 x 10^-2 Ms^-1

The catalyst alters the rate of a chemical reaction by,

• providing an alternative pathway with a lower Ea

• changing the products formed in the direction of the reaction

• providing a surface on which the molecules react

• increasing the frequencies of collisions between molecules

Grinding a seltzer tablet into powder increases the rate of reaction due to...

• increased concentration of reactants
• increased surface area
• increased speed of particles.
• better orientation of reactants

A temperature increase causes the particles

• to slow down

• move faster

• collide higher

• in the right order

A possible rate law for a third overall order of a reaction is __________________

• Rate = k [A]²[B]²
• Rate = k [A][B]³
• Rate = k [A]³ [B]
• Rate = k [A]²[B]

Given the chemical equation, Haber Prosess

N₂(g) + 3H₂ (g) --> 2NH₃ (g)

Based on this reaction, first order for concentration N₂ and zero order for concentration H₂.

Write rate law:

• Rate = K [N₂]¹ [H₂]¹

• Rate = K [N₂]¹

• Rate = K [H₂]⁰

• Rate = K [N₂]¹ [H₂]³

Which of the following is a unit of rate of reaction?

• s^-1

• Ms^-1

• M

• M^-1s^-1

For the reaction below, which of the following is the correct differential rate equation?

NH₃(g) + O₂(g) → NO(g) + H₂O(g)

• $rate\ =\ -\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{\text{d}\left[H_2O\right]}{\text{d}t}$

• $rate\ =\ -\frac{1}{2}\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{1}{3}\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{1}{4}\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{1}{2}\frac{\text{d}\left[H_2O\right]}{\text{d}t}$

• $rate\ =\ \frac{\text{d}\left[NH_3\right]}{\text{d}t}=\frac{\text{d}\left[O_2\right]}{\text{d}t}=-\frac{\text{d}\left[NO\right]}{\text{d}t}=-\frac{\text{d}\left[H_2O\right]}{\text{d}t}$

• $rate\ =\ -\frac{1}{4}\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{1}{5}\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{1}{4}\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{1}{6}\frac{\text{d}\left[H_2O\right]}{\text{d}t}$

Write a balanced chemical equation based on the given differential rate equation:

 $rate\ =\ -\frac{\text{d}\left[C_2H_6\right]}{\text{d}t}=\ -\frac{2}{7}\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{1}{2}\frac{\text{d}\left[CO_2\right]}{\text{d}t}=\frac{1}{3}\ \frac{\text{d}\left[H_2O\right]}{\text{d}t}$  

• C2H6 +  $\frac{2}{7}$  O2  $\rightarrow$   $\frac{1}{2}$   CO2 +  $\frac{1}{3}$   H2O

•   $\frac{1}{2}$   CO2 +  $\frac{1}{3}$   H2O  $\rightarrow$  C2H6 +  $\frac{2}{7}$  O2

• C2H6 +  $\frac{7}{2}$  O2  $\rightarrow$  2 CO2 + 3 H2O

• C2H6 +3 O2  $\rightarrow$  2 CO2 + 3 H2O

For the reaction:

4NH₃(g) + 5O₂(g) → 4 NO(g) + 6H₂O(g)

the rate of disappearance of oxygen is 0.020 M/s. What is the rate of formation of H₂O?

• 0.03 Ms^-1

• 0.02 Ms^-1

• 0.017 Ms^-1

• 0.024 Ms^-1