Answer:
Explanation:
From the given information:
[tex]2NO_2_{(g)} \to 2N_{2(g)} + O_{2(g)}[/tex]
The above reaction is a zero-order reaction.
The rate constant = 0.0067 M-s⁻¹
Suppose the volume of the flask = 4L
Initial Mol of dinitrogen monoxide = 300 mmol
The final mol of dinitrogen monoxide = 150 mmol
The molarity of dinitrogen monoxide = [tex]\dfrac{ \text{number of moles of dinitrogen monoxide }}{\text{volume of flask}}[/tex]
[tex]= \dfrac{300 \ m}{ 4 L}[/tex]
= 0.0075 mmol/L
= 0.0075 L
The final concentration [tex]= \dfrac{150 \ m}{ 4 L}[/tex]
= 0.0375 L
By applying zero order equation
[tex]kt = [A_o] -[At][/tex]
[tex](0.0067)(t) = 0.075 - 0.0375[/tex]
[tex](0.0067)(t) = 0.0375[/tex]
[tex]\mathbf{t = 5.59 \ seconds}[/tex]
