Final answer:
The activation energy is 103 kJ for the gas phase decomposition of dinitrogen pentoxide. To find the temperature at which the rate constant is 0.00110, use the Arrhenius equation: k = A * e^(-Ea/RT). Plug in the values and solve for the temperature.
Step-by-step explanation:
The activation energy is the minimum amount of energy required for a chemical reaction to occur. In the gas phase decomposition of dinitrogen pentoxide, the activation energy is 103 kJ. The reaction produces 2 molecules of nitrogen dioxide (NO₂) and half a molecule of oxygen (O₂). The rate constant is a measure of how fast the reaction occurs.
To find the temperature at which the rate constant is 0.00110, we can use the Arrhenius equation:
k = A * e^(-Ea/RT)
Where:
k is the rate constant
A is the pre-exponential factor
Ea is the activation energy
R is the ideal gas constant
T is the temperature in Kelvin
Given the rate constant (k) at 305 K is 0.00110, we can plug in the values into the equation and solve for the temperature:
0.00110 = A * e^(-103/(8.314 * 305))
From here, we can solve for A:
A = 0.00110 / e^(-103/(8.314 * 305))
Once we have the value of A, we can substitute it back into the original equation and solve for the temperature at which the rate constant is 0.00110.
Learn more about activation energy