Final answer:
The final temperature required for the pressure of an ideal gas to decrease from 2.250 atm to 1.600 atm can be calculated using Amontons's/Gay-Lussac's Law, which indicates that there will be a B) decrease in temperature.
Step-by-step explanation:
To find the final temperature that causes the pressure of an ideal gas to be reduced from 2.250 atm to 1.600 atm, we can apply Amontons's/Gay-Lussac's Law, which states that the pressure of a gas is directly proportional to its temperature when the volume and quantity of the gas are held constant. Given the initial temperature (T1) is 62.00 °C, which is equivalent to 62.00 + 273.15 = 335.15 K, we can set up the direct relationship as follows:
P1/T1 = P2/T2
Substituting in the known values:
2.250 atm / 335.15 K = 1.600 atm / T2
To solve for T2, we can rearrange the equation:
T2 = (1.600 atm * 335.15 K) / 2.250 atm
After performing the calculation, we will get the value of T2 in Kelvin, which can then be converted back to °C by subtracting 273.15.
As a result of the decrease in pressure, we can expect a decrease in temperature, which corresponds to option B) A decrease in temperature.