In Brayden's experiment, the reaction rate at 45 °C is four times faster than at 25 °C and 128 times faster at 95 °C compared to 25 °C. For the NaClO3 decomposition, the time required would be reduced to approximately 12 minutes if heated 20 °C higher.
To address the question about temperature rise and reaction rates in Brayden's scientific experiment, we need to use the given information that the rate of a certain reaction doubles for every 10 °C rise in temperature.
For part (a), moving from 25 °C to 45 °C represents a 20 °C increase. Since the rate doubles every 10 °C, going up by 20 °C means the rate will double twice. The rate at 45 °C is therefore four times the rate at 25 °C.
For part (b), increasing the temperature from 25 °C to 95 °C is a 70 °C increase. That is seven increments of 10 °C, meaning the rate doubles seven times. The rate at 95 °C is thus 27 times the rate at 25 °C, or 128 times faster.
For part 57, if the NaClO3 sample was 90% decomposed in 48 minutes at a certain temperature, heating it an additional 20 °C (which is 2 increments of 10 °C) would double the rate twice.
Thus, the decomposition would occur four times faster. To find the new time, divide the original time by the factor of 4, so it would take approximately 12 minutes for the same decomposition.