Answer:
Kinetic energy decreases as temperature decreases.
Explanation:
From the description that the system at 80°C has longer arrows, or move faster than the system at 20°C, having shorter actors indicating a slower motion, we can conclude that the kinetic energy of a body depends on its temperature.
If the system at 80°C shows a greater kinetic energy (faster motion of particles) than the system at 20°C, it then implies that decreasing the temperature of the body decreases its kinetic energy.
Question:
The options are;
a. 10. mL of 1 M HCl(aq) at 10.oC
b. 10. mL of 1 M HCl(aq) at 25oC
c. 10. mL of 3 M HCl(aq) at 10.oC
d. 10. mL of 3 M HCl(aq) at 25oC
Answer:
The correct option is;
d. 10 mL of 3 M HCl(aq) at 25 °C
Explanation:
Factors that influence the rate of the reaction include;
Concentration and
Temperature
Concentration
An increase in concentration leads to a increased number of interaction among the the reacting components of HCl and iron filings such that the number of effective interaction or the rate of the reaction increases, therefore, a 10 mL 3 M HCl will react faster than a 10 mL of 1 M HCl.
Temperature
When the temperature of the reacting HCl is increased, the energy within the reacting system increases leading to an increase in the number of high energy collisions which results in an increased reaction rate, therefore, HCl at 25 °C will react faster than HCl at 10 °C.
Hence the correct option is 10 mL of 3 M HCl(aq) at 25 °C.
