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Standard VII

Chemistry

Order of Reaction

The decomposi...

Question

The decomposition of azo methane, at a certain temperature according to the equation
$(C H_{3})_{2} N_{2} \to C_{2} H_{6} + N_{2}$ is a first order reaction.
After $40$ minutes from the start, the total pressure developed is found to be $350$ mm Hg in place of initial pressure $200$ mm Hg of azo methane. the value of rate constant $k$ is:

2.88 \times 10^{- 4} s^{- 1}

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1.25 \times 10^{- 4} s^{- 1}

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5.77 \times 10^{- 4} s^{- 1}

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3.52 \times 10^{- 4} s^{- 1}

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Solution

The correct option is C $5.77 \times 10^{- 4} s^{- 1}$
$\begin{matrix} (C H_{3})_{2} N_{2} \to & C_{2} H_{6} + & N_{2} at t=o & 200 & 0 & 0 at t=t & 200 - x & x & x \end{matrix}$
According to the question, $Total pressure (P_{t}) = 200 + x = 350$
$\Rightarrow x = 150$
Since it is first order reaction,
$k = \frac{2.303}{t} l o g (\frac{P_{i}}{P_{t} - P_{i}}) ∴ k = \frac{2.303}{40 \times 60} l o g (\frac{200}{200 - 150})$
$\Rightarrow k = 5.77 \times 10^{- 4} s^{- 1}$

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The correct option is C 5.77×10−4 s−1(CH3)2N2→C2H6+N2at t=o20000at t=t200−xxx According to the question, Total pressure(Pt)=200+x=350 ⇒x=150 Since it is first order reaction, k=2.303tlog(PiPt−Pi)∴k=2.30340×60log(200200−150) ⇒k=5.77×10−4s−1