Question

The following data show the rate constant of a reaction measured at several different temperatures. temperature (k) rate constant (1/s) 3004.17×10-2 3100.122 3200.333 3300.858 3402.09. Use an Arrhenius plot to determine the activation barrier (Ea) for the reaction.

Answer 1

To determine the activation energy (Ea) for the reaction, we can use an Arrhenius plot. By plotting ln(k) against 1/T, we can obtain a straight line with a slope of -Ea/R.

Step-by-step explanation:

To determine the activation energy (Ea) for the reaction, we can use an Arrhenius plot. The Arrhenius equation is given by: k = Ae-Ea/RT. Taking the natural logarithm of both sides of the equation, we get: ln(k) = -Ea/RT + ln(A). By plotting ln(k) against 1/T (where T is the temperature in Kelvin), we can obtain a straight line with a slope of -Ea/R, where R is the gas constant.

In this case, we have the rate constants (k) measured at several different temperatures. We can calculate ln(k) for each temperature and plot it against 1/T. The slope of the line will give us the activation energy (Ea).