NEED HELP
(Combined gas Law) A gas at a pressure of 1.50 atm has a volume of 200 mL.
Calculate the new volume if the pressue changes to 1.20 atm.
Assume constant temperature.
P1V1/T1=P2V2/T2
V2=P1V1/P2
To solve this problem, you can use the combined gas law, which relates the initial and final states of a gas sample under constant temperature. The combined gas law is expressed as:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
- P1 and P2 are the initial and final pressures, respectively.
- V1 and V2 are the initial and final volumes, respectively.
- T1 and T2 are the initial and final temperatures, respectively.
In this case, you are given the initial pressure (P1 = 1.50 atm), the initial volume (V1 = 200 mL), and the final pressure (P2 = 1.20 atm). The temperature is assumed to be constant, so T1 = T2.
To find the final volume (V2), rearrange the formula and substitute the given values:
(P1 * V1) / T1 = (P2 * V2) / T2
Since T1 = T2 (constant temperature), we can cancel out the temperature terms:
P1 * V1 = P2 * V2
Substitute in the known values:
(1.50 atm) * (200 mL) = (1.20 atm) * V2
Now, solve for V2:
V2 = (1.50 atm * 200 mL) / 1.20 atm
V2 = 250 mL
Therefore, the new volume, if the pressure changes from 1.50 atm to 1.20 atm while the temperature remains constant, is 250 mL.