The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300 K is 1.0x10-3 /s and the activation energy Ea = 11.488 kJ/mol, the rate constant at 200 K is ___________ x10-5 /s. (Round off to the nearest Integer).
[Given R = 8.314 J/molK]
The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300 K is 1.0x10-3 /s and the activation energy Ea = 11.488 kJ/mol, the rate constant at 200 K is ___________ x10-5 /s. (Round off to the nearest Integer).
[Given R = 8.314 J/molK]
T? = 300 K; K? = 1 * 10? ³ s? ¹
T? = 200 K; K? =?
E_a = 11.488 kJ/mol
Using Arrhenius equation:
log (K? /K? ) = (E_a / 2.303R) * [ (T? - T? ) / (T? )]
log (K? / 10? ³) = (11.488 * 10³ / (2.303 * 8.314) * [ (-100) / (6 * 10? )]
log (K? / 10? ³) = -1
K? / 10? ³ = 10? ¹
K? = 10? s? ¹ or K? = 10 * 10? s? ¹
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