Differential Rate Equation

When [N] is decreasing at 0.6 M min-1, what is the rate of reaction for 3M +2N  $\rightarrow$   P ?

• 0.3 M min-1

• 0.25 M min-1

• 0.6 M min-1

• 1.2 M min-1

When [B] is decreasing at 0.5 molL-1s-1, how fast is [A] decreasing for A +2B  $\rightarrow$   C ?

• 0.5

• 0.25

• 1.0

• 1.25

Which of the following is NOT the unit for 'time' in reaction rate?

• days

• months

• decades

• none of these above

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

Tags

NGSS.HS-PS1-7

Which of the following is NOT the unit of rate of reaction?

• M s^-1

• mol dm^-3 min^-1

• M^-1 s^-1

• mol L^-1 min^-1

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

• s^-1

• Ms^-1

• M

• M^-1s^-1

For the reaction:

2NH₃(g) → N₂(g) + 3H₂(g)

the rate of disappearance of ammonia is 0.30 M/s. What is the rate of formation of H₂?

• 0.30 Ms^-1

• 0.45 Ms^-1

• 0.20 Ms^-1

• 0.60 Ms^-1

For X + Y  $\rightarrow$   XY, if [XY] is increasing at a rate 0.10 M s-1, predict the rate of depletion of both reactants.

• Both have same rate of depletion.

• Rate of depletion of X is doubled from Y.

• Rate of depletion of X is halved from Y.

• The rate of depletion cannot be determined.

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

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(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