Question

In a study to determine the rate of the following reaction:

2NO(g)+O2​(g)2NO2​(g)
the concentration of NO was 0.0550 M at t = 5.0 s and 0.0225 M at t = 650.0 s. What is the average rate of the reaction during this time period?

Answer 1

The average rate of the reaction 2NO(g) + O2(g) → 2NO2(g) is calculated based on the change in concentration of NO over 645 seconds, which results in an average rate of 5.04×10^-5 M/s.

Step-by-step explanation:

The question asks for the average rate of the reaction 2NO(g) + O2(g) → 2NO2(g) during a specific time period. To calculate the average rate, we use the change in concentration of NO over the time period. We can find the average rate using the formula:

Average Rate = Δ[concentration of NO] / Δtime

The change in concentration of NO (Δ[NO]) is the initial concentration minus the final concentration, which is 0.0550 M - 0.0225 M = 0.0325 M. The change in time (Δt) is the final time minus the initial time, which is 650 s - 5 s = 645 s.

Now, we can calculate the average rate:

Average Rate = 0.0325 M / 645 s = 5.04×10-5 M/s

This is the average rate at which the concentration of NO decreases during the given time period. Remember that the rate of decrease in the reactant's concentration is a positive value, so even though the concentration is decreasing, the rate is expressed as a positive value.