Activation Energy (DP IB Chemistry: HL)

Which of the following statements about the Arrhenius plot are correct? 

1.     The gradient has a value of E_a / R
2.     The intercept on the y-axis is ln A
3.     The Arrhenius plot will give a value for activation energy in J mol^-1

The following information was obtained for the rate constant, k, for a reaction at 25 ^OC

A	Ea	R
2.57 × 109 s–1	96.2 kJ mol–1	8.31 J K–1 mol–1

Which expression correctly represents how to calculate the rate constant, k?

The following experimental data was collected. 

Activation energy, Ea	111 kJ mol–1
Rate constant, k	1.30 x 10-4  mol-1 dm3 s-1
Arrhenius constant, A	4.55 × 1013 mol-1 dm3 s-1

 

Which expression correctly calculates the temperature of the reaction?

Consider the following statements: 

1. Many reactions show a doubling of the rate with a temperature increase of 10K
2. The units of k for a second order reaction are mol^-1 dm³ s^-1
3. In the Arrhenius equation, A relates to the energy requirements of the collisions 

Which statements are correct?

Which graph shows the correct relationship between the rate constant, k, and temperature?

Which of the following statements about the constant A in the Arrhenius equation are correct?

1. It is a steric factor for the fraction of collisions where the particles have the correct mutual orientation
2. It takes into account the energy of the colliding particles
3. It takes into account the number of collisions in a chemical reaction

The following information was obtained for the rate constant, k, for a reaction at 25 ^oC.

 

k	Ea	R
3.46 × 10–8 s–1	96.2 kJ mol–1	8.31 J K–1 mol–1

 

Which expression correctly represents how to calculate the constant, A?

 

Which is the correct expression to calculate the activation energy? (R = 8.31J K^–1 mol^–1)

The rate constant data for a reaction at two different temperatures is shown.

 

Temperature / oC	Rate constant / mol-1 dm3 s-1
5	6.81 x 10-6
35	6.11 x 10-5

 

Using the following equation, which expression is the correct calculation for the activation energy of the reaction, in kJ mol^-1? (R = 8.31J K^–1 mol^–1)

When the temperature increases from 25 ^oC to 55 ^oC, the rate constant for the reaction increases by a factor of 1.45.

Using the equation above, which expression is the correct calculation for the activation energy of the reaction? (R = 8.31J K^–1 mol^–1)