The effect of temperature on the rate of reaction in the catalytic conversion of methane into syngas using nickel as the catalyst can be explained using the Arrhenius equation and the concept of activation energy. The Arrhenius equation is given by:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.In the catalytic conversion of methane into syngas a mixture of carbon monoxide and hydrogen , nickel is used as a catalyst to lower the activation energy of the reaction. This allows the reaction to proceed at a faster rate and at lower temperatures than it would without the catalyst.As the temperature increases, the rate of reaction also increases. This is because the molecules have more kinetic energy at higher temperatures, which increases the likelihood of successful collisions between reactant molecules. Additionally, the exponential term in the Arrhenius equation e^-Ea/RT becomes larger as the temperature increases, which means that the rate constant k also increases. This results in a faster reaction rate.However, it is important to note that there is an optimal temperature range for the catalytic conversion of methane into syngas using nickel as the catalyst. At very high temperatures, the catalyst may become less effective due to sintering or other deactivation processes, which can decrease the overall reaction rate. Additionally, side reactions may become more significant at higher temperatures, leading to the formation of unwanted byproducts.In summary, the rate of reaction in the catalytic conversion of methane into syngas using nickel as the catalyst generally increases with temperature, but there is an optimal temperature range for the reaction to proceed efficiently and selectively.