Explanation:

Activation Energy:
Activation energy (Ea) is the minimum amount of energy required for a chemical reaction to occur. It is the energy barrier that must be overcome for the reactant molecules to transform into product molecules.

Effect of Temperature on Reaction Rate:
Increasing the temperature of a reaction generally increases the reaction rate. This is because an increase in temperature provides more kinetic energy to the reactant molecules, allowing them to move faster and collide with greater energy. As a result, a larger fraction of the collisions will have sufficient energy to overcome the activation energy barrier and lead to a successful reaction.

Rate Constant and Temperature:
The rate of a chemical reaction is determined by the rate constant (k) of the reaction. The rate constant is directly proportional to the reaction rate. The Arrhenius equation describes the relationship between the rate constant and temperature:

k = Ae^(-Ea/RT)

Where:
k = rate constant
A = pre-exponential factor (related to collision frequency and orientation)
Ea = activation energy
R = gas constant
T = temperature (in Kelvin)

Effect of Temperature on Rate Constant:
As per the Arrhenius equation, an increase in temperature leads to an increase in the rate constant. This is because the exponential term of the equation (e^(-Ea/RT)) decreases with increasing temperature. Therefore, a higher temperature will result in a higher rate constant and a faster reaction rate.

Calculation:
In this question, the temperature is raised from 295 to 305 Kelvin. We need to determine the change in the rate of the reaction.

Let's assume the rate constant at 295 K is k1, and at 305 K is k2.

The ratio of the rate constants is given by:

k2/k1 = e^(-Ea/RT2) / e^(-Ea/RT1)

Taking the natural logarithm of both sides to eliminate the exponential term:

ln(k2/k1) = (-Ea/RT2) - (-Ea/RT1) = Ea/R * (1/T1 - 1/T2)

Substituting the given values:

ln(k2/k1) = Ea/R * (1/295 - 1/305)

Since we are interested in the change in the rate of the reaction, we can use the fact that the rate is directly proportional to the rate constant:

(rate2 - rate1) / rate1 = k2 - k1 / k1 = e^(ln(k2/k1)) - 1

Using the above equation and substituting the values, we can calculate the change in the rate of the reaction.

In this case, the correct answer is option B, which suggests that the rate of reaction increased by 100%.

For 10°C rise of temperature the rate is almost doubled,