Answer:
The value of temperature for unanalysed reaction is 456.1 K
Explanation:
Step 1: Data given
The activation energy of uncatalyzed reaction is 75.0 kJ/mol.
The activation energy of catalyzed reaction is 49.0 kJ/mol.
The temperature for catalyzed reaction is 25
°C
<u>Step 2:</u> The balanced equation
2 H2O2(aq) ⟶ 2H2O(l) + O2(g)
<u>Step 3:</u> According to Arrhenius equation:
k = Ae ^ (-Ea/RT)
⇒ with k = the rate constant
⇒ with Ea = the activation energy = 49 kJ/mol
⇒ with R = the universal gas constant = 8.314 J/mol*K
⇒ with T = the temperature = 298 K
For uncatalyzed reaction, the rate constant is calculated as:
k(uncatalyzed) = Ae ^ (-75000/8.314 J/mol*K * T)
k(uncatalyzed) = Ae ^ (-9020.93/T)
For catalyzed reaction, the rate constant is calculated as:
k(catalyzed) = Ae ^ (-Ea(catalyzed)/RT))
⇒ with Ea(catalyzed) = 49000 J/mol
⇒ with T = 298 K
k(catalyzed) = Ae ^ (-49000J/(8.314J/mol *K * 298K))
k(catalyzed) = Ae ^(-19.78)
k(catalyzed) = k(uncatalyzed)
Ae^(-19.78) = = Ae ^ (-9020.93/T)
-19.78 = -9020.93/T
T = -9020.93/-19.78
T = 456.1 K
The value of temperature for unanalysed reaction is 456.1 K
