객관식
The activation energy for the decomposition of HI(g) to H2(g) and I2(g) is 186 kJ/mol. The rate constant at 555 K is 3.52 × 10^-7 L/mol-s. What is the rate constant at 645 K?
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15. Chemical Kinetics
Arrhenius Equation
객관식
Using the Arrhenius Equation, what is the rate constant (k) for the reaction of NO with F2 at a temperature of 298 K?
A
4.56 × 10^6 M⁻¹⋅s⁻¹
B
1.23 × 10^7 M⁻¹⋅s⁻¹
C
2.45 × 10^8 M⁻¹⋅s⁻¹
D
5.67 × 10^8 M⁻¹⋅s⁻¹
검증된 단계별 안내1
Identify the Arrhenius Equation: \( k = A e^{-\frac{E_a}{RT}} \), where \( k \) is the rate constant, \( A \) is the pre-exponential factor, \( E_a \) is the activation energy, \( R \) is the gas constant, and \( T \) is the temperature in Kelvin.
Determine the values needed: You need the activation energy \( E_a \), the pre-exponential factor \( A \), and the temperature \( T \). The temperature is given as 298 K. The values for \( A \) and \( E_a \) are typically provided in the problem or can be found in literature.
Convert the activation energy \( E_a \) to the appropriate units if necessary. It is often given in kJ/mol, so you may need to convert it to J/mol by multiplying by 1000.
Substitute the known values into the Arrhenius Equation. Use \( R = 8.314 \) J/(mol·K) for the gas constant.
Calculate the exponential term \( e^{-\frac{E_a}{RT}} \) and then multiply by the pre-exponential factor \( A \) to find the rate constant \( k \).
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