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JulsSmile [24]
3 years ago
5

The isomerization of methylisonitrile to acetonitrileCH3NC(g)→CH3CN(g)is first order in CH3NC . The rate constant for the reacti

on is 2.34×10−4 s−1 at 489 K .The half-life of the reaction when the initial {\rm [CH_3NC]} is 0.030 M is ________ {\rm s}.A. 1.43×105B. 3.37×10−4C. 4.28×103D. 2.14×103E. 2.96×103
Chemistry
1 answer:
lisabon 2012 [21]3 years ago
4 0

Answer:

Option E, Half life = 2.96\times 10^3\ s

Explanation:

For a first order reaction, rate constant and half-life is related as:

            t_{1/2}=\frac{0.693}{k}

Where,

t_{1/2} = Half life

k = Rate constant

Rate constant given = 2.34\times 10^{-4}\ s^{-1}

t_{1/2}=\frac{0.693}{k}

=\frac{0.693}{2.34 \times 10^{-4}}=2.96\times 10^3\ s

So, the correct option is option E.

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Answer:

Hydrogen is the excess reactant

Nitrogen is the limiting reactant

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Explanation:

The reaction of N₂ with H₂ to produce NH₃ is:

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Hydrogen -Molar mass: 2g/mol-

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As there are 62.5 moles of hydrogen:

<h3>Hydrogen is the excess reactant</h3><h3>Nitrogen is the limiting reactant</h3><h3 />

With nitrogen, the limiting reactant, we determine theoretical moles (Assuming 100% of the reaction occurs) and theoretical yield (In mass):

4.46 moles N2 * (2moles NH3 / 1mol N2) = 8.92 moles of ammonia

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8.92 moles of ammonia * (17g/mol) =

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