Arrhenius Equation

Q. Velocity constant of a reaction at 290 K was found to $3.2\times {10}^{-3}se{c}^{-1}$. When the temperature is raised to 310 K, it will be about:

1. $6.4\times {10}^{-3}$
2. $3.2\times {10}^{-4}$
3. $9.6\times {10}^{-3}$
4. $1.28\times {10}^{-2}$

Q. In terms of the "Collisions Theory of Chemical Kinetics", the rate of a chemical reaction is proportional to:

1. The change in free energy per second
2. The change in temperature per second
3. The number of collisions per second
4. The number of product molecules

Q. He is impressed with your work but he wants you to calculate the value of A also. Calculate the value of A given the same conditions. (The rate constants of the reaction at 500 K and 700 K are $0.02s^{-1}$ and $0.07s^{-1}$ respectively.)

1. 18231 J
2. 12831 J
3. 18431 J
4. 19231 J

Q. Plots showing the variation of the rate constant (k) with temperature (T) are given below. The plot that follows Arrhenius equation is:

1. 
2. 
3. 
4. 

Q. A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be $K_1$ and $K_2$ respectively then

1. $K_2\approx 0.5K_1$
2. $K_2\approx 0.25K_1$
3. $K_2\approx 2K_1$
4. $K_2\approx 4K_1$