객관식
Using the Arrhenius Equation, calculate the activation energy for the decomposition of acetaldehyde, CH3CHO, given that the rate constant is 1.1 × 10⁻² L mol⁻¹ s⁻¹ at 703 K and 4.95 L mol⁻¹ s⁻¹ at 865 K.
800
views
15. Chemical Kinetics
Arrhenius Equation
객관식
Using the Arrhenius Equation, calculate the activation energy (Ea) for the reaction between nitrogen dioxide and carbon monoxide given the rate constants at 701 K and 895 K are 2.57 M⁻¹s⁻¹ and 567 M⁻¹s⁻¹, respectively.
A
1.50 kJ/mol
B
15.0 kJ/mol
C
150 kJ/mol
D
75.0 kJ/mol
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 (8.314 J/mol·K), and \( T \) is the temperature in Kelvin.
Use the two-point form of the Arrhenius Equation to solve for \( E_a \): \( \ln\left(\frac{k_2}{k_1}\right) = \frac{E_a}{R} \left(\frac{1}{T_1} - \frac{1}{T_2}\right) \). Here, \( k_1 = 2.57 \text{ M}^{-1}\text{s}^{-1} \) at \( T_1 = 701 \text{ K} \) and \( k_2 = 567 \text{ M}^{-1}\text{s}^{-1} \) at \( T_2 = 895 \text{ K} \).
Calculate the natural logarithm of the ratio of the rate constants: \( \ln\left(\frac{567}{2.57}\right) \).
Calculate the difference in the inverse of the temperatures: \( \frac{1}{701} - \frac{1}{895} \).
Rearrange the equation to solve for \( E_a \): \( E_a = \frac{R \cdot \ln\left(\frac{567}{2.57}\right)}{\frac{1}{701} - \frac{1}{895}} \). Substitute the values and solve for \( E_a \).
관련 영상
관련 실천
