Nitrogen Dioxide NO2 decomposes upon heating to form nitric oxide and oxygen according to the following equation:

2NO2(g) --> 2NO(g) + O2(g)

At the beginning of an experiment the concentration of nitrogen dioxide in a reaction vessel was 0.113 mol/L. After 60.0 s, the concentration decreased to 0.1076 mol/L. Whatt is the average rate of decomposition of NO2 during this time intervail in mol/(L * s)

can someone help me with this one too please

avg rate = delta C/delta T

delta C is change in concentration
delta T is change in time.

0.113-0.1076 = change in C in molarity.
60 sec = change in time.
divide for the answer.

=-4.5*10e-5

This

Gutdhl

To find the average rate of decomposition of NO2 during the given time interval, you will need to calculate the change in concentration of NO2 and divide it by the time interval.

Step 1: Calculate the change in concentration of NO2
Change in concentration = Final concentration - Initial concentration
Change in concentration = 0.1076 mol/L - 0.113 mol/L
Change in concentration = -0.0054 mol/L

Note: The negative sign indicates a decrease in concentration.

Step 2: Calculate the time interval
The time interval is given as 60.0 s.

Step 3: Calculate the average rate of decomposition
Average rate of decomposition = Change in concentration / Time interval
Average rate of decomposition = -0.0054 mol/L / 60.0 s

Finally, perform the calculation:

Average rate of decomposition = -0.0054 mol/L / 60.0 s = -9.0 x 10^(-5) mol/(L * s)

Therefore, the average rate of decomposition of NO2 during the given time interval is -9.0 x 10^(-5) mol/(L * s).