Using the arrhenius equation
ln(k2/k1) = Ea/R * (1/T1 - 1/T2)
substituting the values in the equation we get
ln(7.30/3.90) = 131000/8.314 * (1/(350+273) - 1/T2)
1/T2 = 0.00156534
T2 = 638.83K = 365.83C
Hence the temperature in celsius scale will be equal to 365.83C
The rate constant of a first-order reaction is 3.90 times 10^-4 s^-1 at 350. degreeC. If...
Ch.19 #4 The rate constant of a first-order reaction is 3.90 x 10-45 at 350°C. If the activation energy is 123 kJ/mol, calculate the temperature at which its rate constant is 9.65 x 10-457. °C
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