The following reaction is a first-order decomposition reaction:

2 N₂O₅(g) → 2 N₂O₄(g) + O₂(g)

The change in concentration of N₂O₅ with time is shown in the following graph:

Determine the average rate of the reaction in the time interval 0-260 s.

When heated at 520 °C, a sample of 2.75 L NO gas having a density of 0.00134 g/mL gradually breaks down into N₂ and O₂ gas. If its rate law is —Δ[NO]/Δt = k[NO]² where k = 0.021/(M•min) at 520 °C, determine the partial pressure of N₂ after 4 hours.

Determine the expression for the reaction rate using the change in concentration of each reactants and products.

Reaction: N₂(g) + 3 H₂(g) → 2 NH₃(g)

Consider the reaction 2 H₂(g) + O₂(g) → 2 H₂O(g)

In a 2.0 L flask, the concentration of H₂(g) went from 0.700 M to 0.330 M during the first 40 s of the reaction. Calculate the mass of H₂O(g) produced in the first 20 s.

The kinetic data for the reaction 2 A → B + C is given below.

Calculate the moles of B formed in the first 40 s of the reaction given that there is initially 2.0 L of A.

The data below shows the rate of disappearance of AB in the following reaction: 

AB + CD → AC + BD

Is the average rate between t = 72.0 min and t = 288.0 min greater than the average rate between t = 36.0 min and t = 144.0 min?