What is the final Celsius temperature if 4.42 L of nitric oxide gas at 35°C is cooled until the volume reaches 1.00 L? Assume the pressure remains constant.
(V1/T1) = (V2/T2)
T must be in kelvin
To find the final Celsius temperature, we can use the combined gas law equation, which relates the initial and final temperature, volume, and pressure of a gas.
The combined gas law equation is:
(P1 x V1) / T1 = (P2 x V2) / T2
Given:
Initial volume (V1) = 4.42 L
Initial temperature (T1) = 35°C
Final volume (V2) = 1.00 L
Pressure remains constant.
First, we need to convert the initial temperature from Celsius to Kelvin, as the gas laws use Kelvin temperature scale.
To convert from Celsius to Kelvin, we add 273.15 to the Celsius temperature:
Initial temperature in Kelvin (T1) = 35 + 273.15 = 308.15 K
Now, we can rearrange the combined gas law equation to solve for the final temperature (T2):
T2 = (P2 x V2 x T1) / (P1 x V1)
Since the pressure remains constant, we can drop the pressure terms from the equation and simplify it to:
T2 = (V2 x T1) / V1
Plugging in the values we have:
T2 = (1.00 L x 308.15 K) / 4.42 L
We can now calculate the final temperature (T2):
T2 = 69.89 K
Finally, converting the final temperature from Kelvin back to Celsius:
Final Celsius temperature = 69.89 K - 273.15 = -203.26°C
Therefore, the final Celsius temperature, when 4.42 L of nitric oxide gas at 35°C is cooled until the volume reaches 1.00 L (with constant pressure) is approximately -203.26°C.