NEET

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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