The temperature of a 4.00 L sample of gas is changed from 10.0 C to 20.0 C. What will the volume of this gas be at the new temperature if the pressure is held constant?
(V1/T1) = (V2/T2)
Don't forget T must be in kelvin.
To find the volume of the gas at the new temperature, we can use the relationship between temperature and volume known as Charles's Law. Charles's Law states that the volume of a gas is directly proportional to its temperature, assuming that the pressure and amount of gas remain constant.
First, let's convert the temperatures from Celsius to Kelvin since Kelvin is the absolute temperature scale. To convert Celsius to Kelvin, we add 273.15 to the Celsius temperature.
Initial temperature (T1) = 10.0 C + 273.15 = 283.15 K
Final temperature (T2) = 20.0 C + 273.15 = 293.15 K
Now, we can write the equation for Charles's Law:
(V1 / T1) = (V2 / T2)
Where:
V1 = Initial volume
T1 = Initial temperature
V2 = Final volume (what we want to find)
T2 = Final temperature
We rearrange the equation to solve for V2:
V2 = (V1 * T2) / T1
Given values:
V1 = 4.00 L
T1 = 283.15 K
T2 = 293.15 K
Substituting the values into the equation, we get:
V2 = (4.00 L * 293.15 K) / 283.15 K
Calculating the result, we find:
V2 = 4.14 L
Therefore, the volume of the gas at the new temperature (20.0 °C) will be approximately 4.14 L, assuming the pressure remains constant.