Final answer:
Reaction order characterizes how reaction rates depend on reactant concentrations and can be influenced by temperature changes. For instance, a reaction that doubles in rate for every 10 °C rise in temperature would proceed four times faster at a 20 °C increase, and 128 times faster after a 70 °C increase. Such temperature-dependent kinetics is pivotal in understanding and controlling chemical reaction rates.
Step-by-step explanation:
The question pertains to the determination of reaction order and how it varies with changes in temperature. Reaction order is a critical concept in kinetics which describes the relationship between the rates of chemical reactions and the concentrations of reactants. To calculate the reaction order with respect to a reactant like sulfuryl chloride, one would typically use experimental data indicating how the rate of the reaction changes with varying concentrations of the reactant while keeping other conditions constant.
Regarding the effects of temperature changes, if a reaction's rate doubles for every 10 °C increase in temperature, this is an example of temperature's influence on reaction kinetics. Specifically, if a reaction proceeds twice as fast at 45 °C compared to 25 °C, it means there has been a 20 °C increase, which corresponds to a fourfold increase in rate (doubling once for each 10 °C increment). Similarly, going from 25 °C to 95 °C results in a 70 °C increase, or a 128 times faster reaction, as the rate doubles seven times (2 to the power of 7).
Finally, if a sample of NaClO3 is 90% decomposed in 48 minutes at a certain temperature and the rate of decomposition doubles with every 10 °C increase, the same level of decomposition would take approximately half as long, or 24 minutes, if the temperature was increased by 20 °C.