14) The rate constant of a first-order reaction is 3.00 × 10^−4 s^−1 at 350.°C. If the activation energy is 149 kJ/mol, calculate the temperature at which its rate constant is 7.60 × 10^−4 s^−1.
_____ *C
Given
k1 = 3.00 10-4 s-1
k2 = 7.60 10-4 s-1
T1 = 350 0C = 350 + 273.15 = 623.15 K
T2 = ?
Ea= 149 kJ/mol = 149000 J/mol
R = 8.314 J/mol.K
Now we have the formula
ln(k2 /k1) = -(Ea/R).(1/T2 - 1/T1 )
by rearranging we get
-Rln(k2 /k1)/ Ea = 1/T2 - 1/T1
-Rln(k2 /k1)/ Ea + 1/T1 = 1/T2
T2 = 1 / {1/T1 - Rln(k2 /k1)/ Ea}
T2 = EaT1 / {Ea - T1R.ln(k2 /k1) }
so by using above values and formula we get
T2 = 149000 J/mol 623.15 K / { 149000 J/mol - 623.15 K 8.314 J/mol.K (ln 7.60 10-4 s-1/3.00 10-4 s-1 )
= 92849350 J.K/mol / { 149000 J/mol - 3590.86)
= 638.53 K
= 638.53 - 273.15
= 365.38 0C
So our asnwer is 365 0C
14) The rate constant of a first-order reaction is 3.00 × 10^−4 s^−1 at 350.°C. If...
The rate constant of a first-order reaction is 3.90 times 10^-4 s^-1 at 350. degreeC. If the activation energy is 131 kJ/mol, calculate the temperature at which its rate constant is 7.30 times 10^-4 s^-1. degreeC
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
12. The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 × 10−10 s−1 at 25°C. Calculate the rate constant at 52.1°C if the activation energy is 116 kJ/mol. _____ ×10^____ s−1 (Enter your answer in scientific notation.) 14. The rate constant of a first-order reaction is 2.75 × 10−4 s−1 at 350.°C. If the activation energy is 101 kJ/mol, calculate the temperature at which its rate constant...
3) The rate constant of a first order reaction is 2.6 x 10+ s' at 255 °C. If the activation energy is 99.9 KJ/mol, calculate the temperature at which its rate constant is 4.8 x 104 sl.
Enter your answer in the provided box. The rate constant of a first-order reaction is 2.35 x 10-45-1 at 350.°C. If the activation energy is 135 kJ/mol, calculate the temperature at which its rate constant is 9.00 x 10-45-1. °c
If a first-order reaction has a rate constant of 2.11 x 10-1 s-1 at a temperature of 22.3°C, what would the value of k be if the reaction temperature has changed to 43.4 °C given the activation energy is 52.9 kJ/mol?
points attempts left Check my work Enter your answer in the provided box. -1 The rate constant of a first-order reaction is 3.00 x 10 s 145 kJ/mol, calculate the temperature at which its rate constant is 7.65 x 10 S at 350.°C. If the activation energy is References eBook & Resources
a certain first-order reaction has a rate constant of 3.00×10−2 s−1 at 23 ∘c. what is the value of k at 67 degrees celsius if Ea= 86 kJ/mol
The first order rate constant for a reaction at 610 oC is 2.79e-03 s-1. If the activation energy for the reaction is 181 kJ/mol, what is the rate constant at 710 oC?
For the first-order reaction: Ag) — Bg) the rate constant is k-6x 104 s-at -10°C, and the activation energy is 64 kJ/mol. What is the rate constant at 20°C? (R-8.314 J/mol x K) 0 a. 6x 10451 b.4.3 x 1045-1 OC. 4.1 x 10851 Od. 1.2 x 10051 Oe-2.2 x 1045-1