Which mechanism is consistent with the facts given about the reaction rate equation-

mechanism (I)
mechanism (II)
both (I) and (II)
neither (I) nor (II)

Solution

Rate is determined by the slow step of the mechanism.

How could the progress of this reaction be best monitored?

by monitoring the colour of the reaction mixture
by titration of \(I_{3}^{-}\) with hypo
by precipitation of I^– with Ag⁺
by monitoring the change in pressure

Solution

\(I_{2} + 2S_{2}O_{3}^{-} \rightarrow 2I^{-} + S_{4}O_{6}^{2-}\)

Solution

When x moles of \(I_{3}^{-}\) form per litre then decrease in concentrations of the reactants are x and 3x.

Solution

As per Arrhenius equation /(K = Ae^{-E_a / RT}), the rate constant increases exponentially with temperature

For a first order reaction A ⟶ P,the temperature (T) dependent rate constant (k) was found to follow the equation log k= –(2000)\(\frac{1}{T}\) + 6.0. The pre-exponential factor A and the activation energy E_a, respectively, are

1.0 × 10⁶ s^-1 and 9.2kJ mol^-1
6.0 s^-1 and 16.6 kJ mol^-1
1.0 × 10⁶ s^-1 and 16.6 kJ mol^-1
1.0 × 10⁶ s^-1 and 38.3 kJ mol^-1

Solution

Under the same reaction conditions, initial concentration of 1.386 mol dm^-3 of a substance becomes half in 40 seconds and 20 seconds through first order and zero order kinetics,respectively. Ratio (k₁ / k₀) of the rate constant for first order(k₁) and zero order (k₀) of the reaction is–

0.5 mol^-1 dm³
1.0 mol d m^-3
1.5 mol d m^-3
2.0 mol^-1 dm

Solution

Consider a reaction aG + bH ⟶ Products. When concentration of both the reactants G and His doubled, the rate increases by eight times. However, when concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is

zero
1
2
3

Solution

The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C, the rate of the reaction increases by about :

10 times
24 times
32 times
64 times

Solution

Since for every 10ºC rise in temperature rate doubles for 50ºC rise in temperature increase in reaction rate= 2⁵ = 32 times

Solution

The time for half life period of a certain reaction A ⟶ Products is 1 hour. When the initial concentration of the reactant ‘A’,is 2.0 mol L^-1, how much time does it take for its concentration to come from 0.50 to 0.25 mol L^-1 if it is a zero order reaction ?

4 h
0.5 h
0.25 h
1 h

Solution

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