Kinetics avg rate and rate law

The tangent to the curve in the plot of concentration vs time allows us to calculate

• Instant rate at 300 s

• instant rate at the beginning of the reaction

• Average rate between 200 s and 400 s

• Average rate for the reaction

Tags

NGSS.HS-PS1-5

For the following reaction

2NO(g) + H₂(g) → N₂(g) + 2H₂O(g)

The rate law is

• rate = [NO][H₂]

• Rate = k[NO]²[H₂]

• Rate = k[NO]²

• The rate law cannot be determined

Tags

NGSS.HS-PS1-5

For a reaction that follows the general rate law, Rate = k[A][B]², what will happen to the rate of reaction if the concentration of B is increased by a factor of 4.00? The rate will

• decrease by a factor of 8.00

• increase by a factor of 16.00

• increase by a factor of 8.00.

• decrease by a factor of 16.00.

Tags

NGSS.HS-PS1-5

What is the overall reaction order for the reaction that has the rate law: Rate = k[O₂] [NO ]²

• First

• Second

• Third

• Zeroth

Tags

NGSS.HS-PS1-5

If you increase the temperature of a system, the rate of reaction

• Increases

• Decreases

Tags

NGSS.HS-PS1-5

The average rate of a reaction is defined as

• Δ(mass)/Δt

• Change in concentration

• Δ[concentration]/Δt

• Δt/Δ[concentration]

Tags

NGSS.HS-PS1-5

For the following reaction

2 N₂O₅(g) → 4 NO₂(g) + O₂(g) what is the relationship between the rate of consumption of N₂O₅ and that of appearance of O₂?

• 1/2 Δ[N₂O₅]/Δt = Δ[O₂]

• -1/2 Δ[N₂O₅]/Δt = Δ[O₂]

• -Δ[N₂O₅]/Δt = 1/2 Δ[O₂]

• -Δ[N₂O₅]/Dt = Δ[O₂]

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7

For the following reaction

2 N₂O₅(g) → 4 NO₂(g) + O₂(g)

If the rate of appearance of O₂ is equal to 3.00 mol/min at a particular moment, what is the rate of disappearance of N₂O₅ at that moment?

• 0.750 mol/min

• 1.50 mol/min

• 6.00 mol/min

• 12.0 mol/min