Answer: The concentration of [tex]N_2O[/tex] in three significant figures will be 0.899 mol/L.
Explanation:
For the given reaction:
[tex]2N_2O\rightarrow 2N_2+O_2[/tex]
The above reaction follows zero order kinetics. The rate law equation for zero order follows:
[tex]k=\frac{1}{t}([A_o]-[A])[/tex]
where,
k = rate constant for the reaction = [tex]6.28\times 10^{-3}\text{ mol }L^{-1}s^{-1}[/tex]
t = time taken = 10 sec
[tex][A_o][/tex] = initial concentration of the reactant = 0.962 mol/L
[A] = concentration of reactant after some time = ?
Putting values in above equation, we get:
[tex]6.28\times 10^{-3}=\frac{1}{10}(0.962-[A])[/tex]
[tex][A]=0.899mol/L[/tex]
Hence, the concentration of [tex]N_2O[/tex] in three significant figures will be 0.899 mol/L.
The concentration will be equal to 0.899 mol/L.
The value of "A" will be found as follows:
[tex]6.28*10^-^3=\frac{1}{10} (0.962-[A])\\A= 0.899 mol/L[/tex]
It is important to remember that the concentration of a chemical solution refers to the amount of solute that exists within the solvent.
More information about concentrations at the link:
https://brainly.com/question/14464650
