The pressure of a gas having volume 1800ml. Originally occupying 300ml. at 6 atms. Pressure.
V1=300ml
V2=1800ml
P1=6atm
P2=p
V1×P1=V2×P2
300×6=1800×p
300×6\1800=p
=0atm
P2=0atm
To calculate the pressure of a gas, you can use the ideal gas law equation: PV = nRT. In this equation, P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents temperature.
Given:
Initial volume (V1) = 300ml
Final volume (V2) = 1800ml
Initial pressure (P1) = 6 atm
To find the final pressure (P2), we need to assume that the amount of gas (n) and temperature (T) remain constant. This means that the number of moles and the temperature of the gas do not change.
Here's how you can calculate the final pressure:
Step 1: Convert the volumes to liters since the ideal gas constant (R) is in the units of liters.
Initial volume (in liters): V1 = 300ml = 0.3 liters
Final volume (in liters): V2 = 1800ml = 1.8 liters
Step 2: Apply the ideal gas law equation and solve for the final pressure (P2):
(P1) x (V1) = (P2) x (V2)
Using the values we have:
(6 atm) x (0.3 L) = (P2) x (1.8 L)
Step 3: Solve for P2:
(6 x 0.3) / 1.8 = P2
1 atm = P2
So, the final pressure (P2) of the gas is 1 atm.
To find the final pressure of the gas, we can use Boyle's law, which states that the pressure of a gas is inversely proportional to its volume when the temperature and amount of gas remain constant.
Boyle's law formula:
P1V1 = P2V2
Where:
P1 = Initial pressure (6 atm)
V1 = Initial volume (300 ml)
P2 = Final pressure (unknown)
V2 = Final volume (1800 ml)
We can rearrange the formula to solve for P2:
P2 = (P1 * V1) / V2
Plugging in the values:
P2 = (6 atm * 300 ml) / 1800 ml
Calculating:
P2 = 1800 atm*ml / 1800 ml
Simplifying the units:
P2 = 1 atm
Therefore, the final pressure of the gas is 1 atm.