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प्रश्न
Consider figure and mark the correct option.
विकल्प
Activation energy of forward reaction is E1 + E2 and product is less stable than reactant.
Activation energy of forward reaction is E1 + E2 and product is more stable than reactant.
Activation energy of both forward and backward reaction is E1 + E2 and reactant is more stable than product.
Activation energy of backward reaction is E1 and product is more stable than reactant.
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उत्तर
Activation energy of forward reaction is E1 + E2 and product is less stable than reactant.
Explanation:
Ea (forward) = E1 + E2
Since energy of reactants is less than products and the product is less stable than the reactant.
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संबंधित प्रश्न
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`logk=logA-E_a/2.303R(1/T)`
Where Ea is the activation energy. When a graph is plotted for `logk Vs. 1/T` a straight line with a slope of −4250 K is obtained. Calculate ‘Ea’ for the reaction.(R = 8.314 JK−1 mol−1)
The rate constant of a first order reaction increases from 2 × 10−2 to 4 × 10−2 when the temperature changes from 300 K to 310 K. Calculate the energy of activation (Ea).
(log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)
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| T/°C | 0 | 20 | 40 | 60 | 80 |
| 105 × k/s−1 | 0.0787 | 1.70 | 25.7 | 178 | 2140 |
Draw a graph between ln k and `1/T` and calculate the values of A and Ea. Predict the rate constant at 30º and 50ºC.
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The reaction must be:
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Which plot of ln k vs `1/T` is consistent with the Arrhenius equation?
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