NEET2026ChemistryChapterActual
The given figure displays the Arrhenius plots ( k vs 1 T ) for two distinct chemical reactions, labeled as Reaction X and Reaction Y. Based on the provided graph, identify the correct relationship between their activation energies ( E_a ).
Options
- AE_a of Reaction X < E_a of Reaction Y
- BE_a of Reaction X > E_a of Reaction Y
- CE_a of Reaction X = E_a of Reaction Y
- DActivation energy cannot be compared without knowing the exact temperature range.
Correct answer
B. E_a of Reaction X > E_a of Reaction Y
Step-by-step solution
According to the Arrhenius equation: k = A e^ -E_a / RT Taking the natural logarithm on both sides, we get: k = A - E_a R ( 1 T ) This represents a straight line equation y = mx + c , where the y-axis is k and the x-axis is 1 T . The slope of the line is given by m = - E_a R . From the given graph, the line for Reaction X is steeper (more negative) than the line for Reaction Y. This means the magnitude of the slope for Reaction X is greater than that for Reaction Y. | m_X | > | m_Y | E_ a,X R > E_ a,Y R E_ a,X > E_