The volume of a gas is 17.7 mL at 41◦C and
0.819 atm. What will the volume be at 16◦C
and 0.996 atm?
Answer in units of mL
(P1V1/T1) = (P2V2/T2)
Remember T must be in kelvin.
6.66
To solve this question, we can use the combined gas law formula, which relates the initial volume (V1), initial temperature (T1), initial pressure (P1), and the final volume (V2), final temperature (T2), and final pressure (P2).
The formula for the combined gas law is:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Given:
V1 = 17.7 mL
T1 = 41°C (convert to Kelvin by adding 273.15, so T1 = 41 + 273.15 = 314.15 K)
P1 = 0.819 atm
T2 = 16°C (convert to Kelvin, so T2 = 16 + 273.15 = 289.15 K)
P2 = 0.996 atm
Now, we can plug in these values into the combined gas law formula:
(0.819 atm * 17.7 mL) / (314.15 K) = (0.996 atm * V2) / (289.15 K)
Next, we can solve for V2, which is the final volume:
V2 = [(0.819 atm * 17.7 mL) / (314.15 K)] * (289.15 K / 0.996 atm)
Calculating this equation will give us the final volume (V2) in units of mL.
Note: Make sure to convert the temperatures to Kelvin before plugging them into the formula.