Question

The first-order rate constant for the reaction of methyl chloride (ch3cl) with water to produce methanol (ch3oh) and hydrochloric acid (hcl) is 3.32 x 10 -10 s -1 at 250c. calculate the rate constant at 400c if the activation energy is 116 kj/mol.

Answer 1

Using the Arrhenius equation and the given activation energy, one can calculate the rate constant at 400°C for the reaction involving methyl chloride and water.

Step-by-step explanation:

The student has asked to calculate the rate constant at 400°C for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) given that the first-order rate constant at 25°C is 3.32 x 10-10 s-1 and the activation energy is 116 kJ/mol. To solve this, we use the Arrhenius equation which relates the rate constant (k), the activation energy (Ea), and the temperature (T).

The Arrhenius equation in logarithmic form is ln(k2/k1) = (Ea/R) * ((1/T1) - (1/T2)), where k1 and k2 are the rate constants at temperatures T1 and T2 respectively, Ea is the activation energy, and R is the gas constant (8.314 J/mol·K).

By solving this equation using the provided values and temperatures converted to Kelvin (298.15K for 25°C and 673K for 400°C), we can calculate the rate constant k2 at 400°C.