The temperature of a 2.25L sample of gas decreases from 45.0'C to 20.0'C. What is the new volume?
(V1/T1) = (V2/T2)
Remember T must be in kelvin.
so then would the answer be 2.07?
2.07L, yes.
ok thanks a lot for your help :D
To find the new volume of the gas sample, we can use the ideal gas law formula, which states:
PV = nRT
Where:
- P is the pressure of the gas (which is assumed to be constant),
- V is the volume of the gas,
- n is the number of moles of gas (which is also assumed to be constant),
- R is the ideal gas constant, and
- T is the temperature of the gas in Kelvin.
To solve for the new volume, we need to convert the temperatures from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature.
Given:
Initial temperature (Ti) = 45.0°C
Final temperature (Tf) = 20.0°C
Initial volume (Vi) = 2.25 L
First, let's convert the temperatures to Kelvin:
Ti = 45.0°C + 273.15 = 318.15 K
Tf = 20.0°C + 273.15 = 293.15 K
Next, we can set up the equation using the ideal gas law:
(Pi)(Vi) / Ti = (Pf)(Vf) / Tf
Since the pressure and number of moles are assumed to be constant, we can simplify the equation to:
Vi / Ti = Vf / Tf
Now, plug in the values:
2.25 L / 318.15 K = Vf / 293.15 K
Now, cross-multiply and solve for Vf:
(2.25 L) * (293.15 K) = Vf * (318.15 K)
Vf = (2.25 L * 293.15 K) / 318.15 K
Vf ≈ 2.072 L
Therefore, the new volume of the gas sample is approximately 2.072 L.