The number of correct statement/s from the following is _____ .A.Larger the activation energy, smaller is the value of the rate constant.B. The higher is the activation energy, higher is the value of the temperature coefficient.C. At lower temperatures, increase in temperature causes more change in the value of k than at higher temperature.D. A plot of ln k vs 1 T is a straight line with slope equal to −EaR

Let's evaluate each statement one by one:

A. Larger the activation energy, smaller is the value of the rate constant. This statement is correct. The rate constant (k) is inversely proportional to the activation energy. This is because a larger activation energy means that more energy is required for the reaction to occur, which slows down the rate of the reaction.

B. The higher is the activation energy, higher is the value of the temperature coefficient. This statement is also correct. The temperature coefficient (usually denoted by Q10) is a measure of how much the rate of a reaction increases with a 10°C increase in temperature. If the activation energy is higher, it means that the reaction is more sensitive to temperature changes, so the temperature coefficient will be higher.

C. At lower temperatures, increase in temperature causes more change in the value of k than at higher temperature. This statement is correct as well. The rate constant k increases with temperature, but the relationship is not linear. At lower temperatures, a small increase in temperature can cause a large increase in k. But at higher temperatures, the same increase in temperature will cause a smaller increase in k.

D. A plot of ln k vs 1 T is a straight line with slope equal to −Ea/R This statement is also correct. This is known as the Arrhenius equation, which describes the temperature dependence of reaction rates. The slope of the plot of ln k vs 1/T is equal to the negative of the activation energy divided by the gas constant R.

So, all four statements are correct. Therefore, the number of correct statements is 4.