Answer:
The rate constant at T = 100 C is 1.0*10⁻³
Explanation:
The Arrhenius equation relates two rate constants K1 and K2 measured at temperatures T1 and T2 as shown below:
[tex]ln\frac{K_{2}}{K_{1}}=\frac{\Delta H^{0}rxn}{R}(\frac{1}{T_{1}}-\frac{1}{T_{2}})[/tex]
here, ΔHrxn = standard enthalpy change of the reaction
R = gas constant
From the given information:
K1 = 7.4*10^-4
T1 = 25 C = 25+273 = 298 K
T2 = 100 C = 100+273 = 373K
ΔH°=4.1kJ/mol
[tex]ln\frac{K_{2}}{7.4*10^{-4}}=\frac{4.1 kJ/mol}{0.08314kJ/mol.K}(\frac{1}{298}-\frac{1}{373})K[/tex]
K2 = 1.03*10⁻³
