Reaction Order
[A]₀ Initial1.00 M
Activation Energy Ea50 kJ/mol
Frequency factor A10^13
Temperature298 K (25°C)
Molar mass (MB dist.)28 g/mol
All Values
k (rate const.)17198.1653 s⁻¹
t½ (half-life)4.03e-5 s
[A] current1.0000 M
Rate current1.72e+4 M/s
% remaining100.0 %
ln k9.75
Ea/R6014 K
Rate Law
rate = k[A] (first order — rate ∝ [A])
Integrated Rate Law
📐 ln[A] = ln[A]₀ − kt
[A] = [A]₀·e^(−kt)
Graph: ln[A] vs t → straight line, slope = −k
Formulas for k
k = ln([A]₀/[A]) / t
k = 2.303 × log([A]₀/[A]) / t ← JEE form
k = ln 2 / t½ = 0.693 / t½
k = (1/t) × ln(N₀/N) (for radioactive decay)
Units: s⁻¹ (time⁻¹)
Half-life (t½)
⏱ t½ = ln2 / k = 0.693 / k
t½ independent of [A]₀ ← KEY JEE fact!
λ = k (decay constant) for radioactivity
k calc: —
Reaction Progress — 1st Order[A] = 1.0000 M rate = 1.72e+4 M/s
0%100% remaining t = 0.0s t½ = 4.03e-5s100%
Exponential decay — use ln[A] vs t for linearity