The volume of a gas is increased from 100mL to 250 mL by heating it.If the original temperture of the gas was 15.0°c what will be the final temperture in °c
(V1/T1) = (V2/T2)
Remember T must be in kelvin
the volume increased by a factor of 2.5
the volume is directly proportional to the absolute (Kelvin) temperature
ºK = ºC + 273
To find the final temperature of the gas, you can use the combined gas law equation, which relates the initial and final volumes and temperatures of a gas.
The combined gas law equation is:
(P1 × V1) / T1 = (P2 × V2) / T2
Where:
P1 = initial pressure (which is not given in this case, so it's not needed)
V1 = initial volume (100 mL, or 0.1 L)
T1 = initial temperature (15.0°C, or 15.0 + 273.15 = 288.15 K)
V2 = final volume (250 mL, or 0.25 L)
T2 = final temperature (what we need to find)
Now, rearrange the equation to solve for T2:
T2 = (T1 × (P2 × V2)) / (P1 × V1)
Since the pressure remains constant in this case, we can remove it from the equation:
T2 = (T1 × V2) / V1
Plug in the known values:
T2 = (288.15 K × 0.25 L) / 0.1 L
T2 ≈ 720.375 K
To convert the final temperature from Kelvin back to Celsius, subtract 273.15:
T2 ≈ 720.375 - 273.15 ≈ 447.225°C
Therefore, the final temperature of the gas will be approximately 447.225°C.