A 2.50-L volume of hydrogen measured at -100 degrees Celsius is warmed to 100 degrees Celsius. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.
(V1/T1) = (V2/T2)
Remember T1 and T2 must be in kelvin. K = 273 + C
You know V1, T1 and T2. Substitute and solve for V2.
Post your work if you get stuck.
A 2.5 L volume of hydrogen gas measured at -196 degrees Celsius is warmed to 100 degrees Celsius. Calculate the volume of the gas at the "higher" temperature, assuming no change in pressure.
To solve this problem, we can use Charles's Law, which states that the volume of an ideal gas is directly proportional to its temperature, assuming that the pressure and the number of particles remain constant.
To calculate the volume of the gas at a higher temperature, we need to find the ratio between the initial and final temperatures and apply this ratio to the initial volume.
First, let's convert the temperatures from Celsius to Kelvin. To convert from Celsius to Kelvin, we add 273.15 to the Celsius temperature.
Initial temperature (T1) = -100°C + 273.15 = 173.15 K
Final temperature (T2) = 100°C + 273.15 = 373.15 K
Next, let's set up the ratio:
(Volume at T2) / (Volume at T1) = (Temperature at T2) / (Temperature at T1)
(Volume at T2) / (2.50 L) = (373.15 K) / (173.15 K)
Now, solve for the volume at T2:
(Volume at T2) = (2.50 L) * (373.15 K) / (173.15 K)
Calculating this expression will give us the volume of the gas at the higher temperature.