Question bank/NEET UG/Chemistry

NEET UGChemistryModerateRe-NEET 2026

For an elementary chemical reaction, the Arrhenius plot is given below.
[IMAGE]
If the energy of activation is 6.64 kJ mol⁻¹ and R = 8.3 J K⁻¹ mol⁻¹, the temperature at which the rate constant becomes e² min⁻¹, is

Show answer and solution
Sol. lnk=lnA−EaRTlnk = lnA - \frac{E_a}{RT}
ln(e2)=6−6.64×103J mol−18.3 J K−1 mol−1×Tln(e^2) = 6 - \frac{6.64 \times 10^3 J~mol^{-1}}{8.3~J~K^{-1}~mol^{-1} \times T}
2=6−6.64×1038.3×T2 = 6 - \frac{6.64 \times 10^3}{8.3 \times T}
T=6.64×1038.3×4=200T = \frac{6.64 \times 10^3}{8.3 \times 4} = 200 K

Source: geekyrakshit/indian-exam-questions / reneet2026-code50

More NEET UG questionsChapter practice

Need a video for this idea?

Scan any doubt from your notes and get a whiteboard explanation.

Scan a doubtView plans