What is the final volume of 725 mL of neon gas at 240.°C if the gas is cooled to 54.5°C? Assume the pressure and the amount of gas are held constant.
v1- 725/100 = .725
v2 - unknown
t1- 240 C +273 K (to convert celcius to kelvin
t2 - 54.5 C + 273 K
V2 = .725 x 327.5 / 513
v2 = .462841
V2= .46
v1- 725/100 = .725
should be 725/1000; otherwise ok through the problem. At the end, V2 should be rounded to 0.463 and the unit should be L.
yep forgot the units sorry.
To find the final volume of the neon gas, we can use Charles' Law, which states that the volume of a gas is directly proportional to its temperature, as long as the pressure and the amount of gas are held constant.
Charles' Law can be expressed as:
V1 / T1 = V2 / T2
Where:
V1 is the initial volume of the gas,
T1 is the initial temperature of the gas in Kelvin,
V2 is the final volume of the gas,
T2 is the final temperature of the gas in Kelvin.
First, let's convert the initial and final temperatures from Celsius to Kelvin. The Kelvin scale starts from absolute zero and is offset by 273.15 degrees from the Celsius scale.
Initial temperature (T1) = 240°C + 273.15 = 513.15 K
Final temperature (T2) = 54.5°C + 273.15 = 327.65 K
Now, we can plug these values into Charles' Law:
V1 / T1 = V2 / T2
Solving for V2:
V2 = V1 * (T2 / T1)
Given:
V1 = 725 mL (initial volume)
Using the formula, we can calculate the final volume:
V2 = 725 mL * (327.65 K / 513.15 K)
V2 = 725 mL * 0.638
V2 ≈ 462.35 mL
Therefore, the final volume of the neon gas, when cooled from 240°C to 54.5°C, is approximately 462.35 mL.