A reaction has an activation energy, Ea = 41.6 kJ mol-1 at 25 °C. By how many degrees must the temperature be raised in order to increase the reaction rate by a factor of 30.
2.0
6.0
C. 29
374
76
The following reaction takes place in an acidic solution
As4O6(s) + MnO4-(aq) → AsO43-(aq) + Mn2+(aq)
In the simplest balanced equation, the coefficients for each listed species are
As4O6 MnO4- H+
1,3,12
B. 3,5,36
5,8,36
5,8,30
2,3,5
1)
Given:
T1 = 25 oC
=(25+273)K
= 298 K
K2/K1 = 30/1
Ea = 41.6 KJ/mol
= 41600 J/mol
use:
ln(K2/K1) = (Ea/R)*(1/T1 - 1/T2)
ln(30/1) = (41600.0/8.314)*(1/298 - 1/T2)
3.4012 = 5003.6084*(1/298 - 1/T2)
T2 = 374 K
= (374-273) oC
= 101 oC
Increase in temperature = T2 - T1
= 101 oC - 25 oC
= 76 oC
Answer: E
Only 1 question at a time please
A reaction has an activation energy, Ea = 41.6 kJ mol-1 at 25 °C. By how...
A reaction has an activation energy, Ea = 41.6 kJ mol-1 at 25 °C. By how many degrees must the temperature be raised in order to increase the reaction rate by a factor of 30. A) 2.0 B) 374 C) 29 D) 76 E) 6.0
2) Draw reaction energy diagram if this reaction has an activation energy (Ea) of +17 kJ/mol.
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