Methyl Isonitrile Rearrangement Quiz

The minimum energy that molecules must possess to react. It is a measure of the energy barrier for the reaction.

The relationship between the rate constant (k) and temperature (T) is given by the Arrhenius equation: k = Ae^(-Ea/RT), where A is the pre-exponential factor, R is the gas constant, and Ea is the activation energy.

The rate constant (k) is a measure of the reaction rate at a specific temperature. It is related to the activation energy (Ea) by the Arrhenius equation.

The natural logarithm of the rate constant (k) is directly proportional to the reciprocal of the absolute temperature (1/T). This relationship is expressed by the Arrhenius equation.

The activation energy (Ea) can be determined from the slope of the linear plot of ln(k) versus 1/T. The slope is equal to -Ea/R, where R is the gas constant.

The pre-exponential factor (A) is a constant in the Arrhenius equation that accounts for the frequency of collisions between molecules. It reflects the likelihood that a collision will lead to a reaction.

The rate constant (k) changes with temperature. This is due to the exponential relationship between k and temperature in the Arrhenius equation. Higher temperatures lead to a faster reaction due to increased molecular collisions and more molecules having sufficient energy to overcome the activation energy.

The Arrhenius equation can be used to predict the rate constant at a different temperature. The equation can be rearranged to solve for the rate constant (k) at a specific temperature (T) if you know the activation energy (Ea), the pre-exponential factor (A), and the gas constant (R).

The experimental values of k are used to calculate the activation energy (Ea) using the Arrhenius equation.

The value of the rate constant (k) at a different temperature (430.0 K) can be calculated using the Arrhenius equation and the previously calculated activation energy (Ea).