In the first 14.0 s of the reaction, 1.7×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.340 L What is the average rate of the reaction over this time interval? 2 N2O(g) → 2 N2(g)+O2(g)
time = 14 s
change in O2 = 0.017 mols.
volume = 0.340 L
[O2] = mols/L = 0.017/0.340 = estimated 0.05 M
rate = 0.05M/14 s = ?
Well, it seems like we have some chemistry going on here! Let me calculate the average rate of the reaction for you, but be prepared for my clownish response!
So, to find the average rate, we need to divide the change in the amount of O2 by the change in time. In this case, we have 1.7×10^(-2) mol of O2 produced in a time interval of 14.0 s.
Calculating the average rate: 1.7×10^(-2) mol / 14.0 s = 0.0012 mol/s.
Voila! The average rate of the reaction is 0.0012 mol/s. That's as fast as a snail on roller skates! Keep those reactions rollin'!
To find the average rate of the reaction, you need to calculate the change in the concentration of O2 over the given time interval. The average rate of a reaction is defined as the change in concentration divided by the change in time.
Given:
- Time interval: 14.0 seconds
- Moles of O2 produced: 1.7 × 10^(-2) mol
- Volume of the reaction vessel: 0.340 L
To find the average rate, we need to convert the moles of O2 to concentration. Concentration is expressed as moles of a substance per liter of solution (M):
Concentration (M) = moles of O2 / volume of reaction vessel
Concentration (M) = (1.7 × 10^(-2) mol) / (0.340 L)
Now, let's substitute the given values:
Concentration (M) = 0.050 mol/L
To calculate the average rate, we divide the change in concentration by the change in time:
Average rate = change in concentration / change in time
Change in concentration = final concentration - initial concentration
In this case, the initial concentration of O2 is zero because it is produced over the reaction time interval. The final concentration is 0.050 M.
Change in concentration = (0.050 M) - 0
Change in concentration = 0.050 M
Now, let's substitute the values into the formula:
Average rate = (0.050 M) / (14.0 s)
Average rate ≈ 0.0036 M/s
Therefore, the average rate of the reaction over the first 14.0 s is approximately 0.0036 M/s.
To find the average rate of the reaction, we need to determine the change in concentration of the reactant or product over the given time interval.
In this case, we are given the amount of O2 produced, which is 1.7×10^−2 mol, and the reaction volume, which is 0.340 L.
To calculate the concentration of O2, we divide the amount of O2 by the volume of the reaction vessel:
Concentration of O2 = (1.7×10^−2 mol)/(0.340 L)
Next, we need to determine the average rate of the reaction. The rate is defined as the change in concentration of a reactant or product divided by the time it takes for that change to occur.
In this case, the time interval is given as 14.0 s. Therefore, we can calculate the average rate of the reaction by dividing the change in concentration of O2 by the time interval:
Average rate = (Concentration of O2)/(Time interval)
By substituting the given values into the equation, we can calculate the average rate of the reaction.