Class XII Chemistry Chemical Kinetics 4

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Question 1

Initial temperature is 37 °C. If E_a is 50kJ/mol, by what factor is the increase when its temperature changes to 40 °C?

• A0.2
• B1.145
• C1.6
• D2.0

Question 2

According to the collision theory of reaction rates, an increase of the temperature at which the reaction occurs will in turn increase rate of reaction. This is caused due to:

• AGreater number of molecules are having the activation energy(threshold energy)
• BGreater velocity of reaction molecules
• CGreater number of collisions
• DNone of these

Question 3

for the reaction A⟶ B, data of initial concentration and corresponding half-life period are given in the tabular form

The order of the reaction is

• A0
• B1
• C2
• D3

Question 4

A first order reaction follows the expressions

• AC_t e^kt = C₀
• BC_t = C₀ e^kt
• CLn C₀/C_t = -k_t
• DLn C_t/C₀ = k_t

Question 5

units of rate constant of zero order reactions in terms of molarity unit are respectively

• AM sec^-1
• BM
• CM sec
• Dsec^-1

Question 6

the rate law for the reaction
RCl + NaOH(aq.)⟶ ROH + NaCl is given by
Rate = k₁ [RCl]. The rate of the reaction will be

• Adoubled on doubling the concentration of NaOH
• Bhalved on reducing the concentration of RCl to one half
• Cdecreased on increasing the temperature of the reaction
• Dunaffected by increasing the temperature of the reaction

Question 7

When a graph between ln K and 1/T is drawn a straight line is obtained. The point at which line cuts y -axis and x -axis respectively correspond to the temp?

• A0, Ea / 2.303 R log A
• Bln A, R (ln A)/E
• C0, log A
• DNone of these

Question 8

The decomposition of N₂O into N₂ & O₂ in presence of gaseous argon follow second order kinetics with k = (5.0 × 10¹¹) e^-41570/T. The energy of activation of the reaction is?

• A5.0 x 10¹¹ J
• B41570 J
• C345612.98 J
• Dnone

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