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Standard XII

Chemistry

Basic Buffer Action

Assuming ∙ ...

Question

Assuming $∙ C H_{3} a n d ∙ C H_{3} C O$ to be under steady state (i.e. the rate of formation and rate of consumption of an intermediate species are equal), derive expressions for $(i) [∙ C H_{3}] a n d (i i) [∙ C H_{3} C O]$ in terms of $[C H_{3} C H O]$ .

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Solution

$i) \frac{d [{C H}_{3}]}{d t} = k_{1} [{C H}_{3} C H O] - k_{2} [{C H}_{3} C H O] [{C H}_{3}] + k_{3} [{C H}_{3} C O] - 2 k_{4} {[{C H}_{3}]}_{3}^{2} = 0 i i) \frac{d [{C H}_{3} C O]}{d t} = k_{2} [{C H}_{3} C H O] [{C H}_{3}] - k_{c} [{C H}_{3} C O] = 0 [{C H}_{3}] = \sqrt \frac{k_{1}}{{2 k}_{4}} {[{C H}_{3} C H O]}_{3}^{1 / 2} [{C H}_{3} C O] = \frac{k_{2}}{k_{3}} \sqrt \frac{k_{1}}{{2 k}_{4}} {[{C H}_{3} C H O]}_{3}^{1 / 2}$

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Similar questions

Q. In the photochemical decomposition of acetaldehyde, one photon of absorbed light decomposes one molecule of

C H_{3} C H O

into

∙ C H_{3} a n d ∙ C H O

. If

^{'} I_{a b s}^{'}

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Calculate

[∙ C H_{3}] a n d \frac{d [C O]}{d t}

assuming steps (ii) to (iv) given are same and

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are under steady state.

Q. Which of the following reagent cannot be used for differentiation between

C H_{3} C H O

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Q. For the mechanism

A + B k_{1} - \to k_{2} C

C_{3} D

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k_{3} << k_{2}

, express the pre-exponential factor A and

E_{a}

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A_{1}, A_{2} a n d A_{3} a n d E_{a_{1}}, E_{a_{2}} a n d E_{a_{3}}

for the three steps.

Q. The decomposition of dimethyl ether leads to the formation of

C H_{4}, H_{2}

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K (p_{C} H_{3} O C H_{3})^{\frac{3}{2}}

If pressure is measured in bar and time in minutes, the units of rate constant are

The decomposition of dimethyl ether leads to the formation of CH₄, H₂ and CO and the reaction rate is given by

Rate = k [CH₃OCH₃]^3/2

The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,

If the pressure is measured in bar andtime in minutes, then what are the units of rate and rate constants?

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Assuming ∙CH3and∙CH3CO to be under steady state (i.e. the rate of formation and rate of consumption of an intermediate species are equal), derive expressions for (i) [∙CH3] and (ii) [∙CH3CO] in terms of [CH3CHO].

i)d[CH3]dt=k1[CH3CHO]−k2[CH3CHO][CH3]+k3[CH3CO]−2k4[CH3]2=0ii)d[CH3CO]dt=k2[CH3CHO][CH3]−kc[CH3CO]=0[CH3]=√k12k4[CH3CHO]1/2[CH3CO]=k2k3√k12k4[CH3CHO]1/2

Assuming $∙ C H_{3} a n d ∙ C H_{3} C O$ to be under steady state (i.e. the rate of formation and rate of consumption of an intermediate species are equal), derive expressions for $(i) [∙ C H_{3}] a n d (i i) [∙ C H_{3} C O]$ in terms of $[C H_{3} C H O]$ .