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Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of :
0.0067·Ms−1: 2N2O(g)→2N2(g)+O2(g)
Suppose a flask is charged under these conditions with of ammonia. After how much time is there only left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to significant digits.

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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]

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