10.7L of a gas at 1.75 atm are expanded to 20.0L at a mass constant temperature.what the new gas pressure?
Assume ideal gas law
PV = nRT
Since the question mentions constant mass and temperature, P1V1 = P2V2
(1.75)(10.7) = P2(20.0L)
P2 = ?
To find the new gas pressure, we can use the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature (assumed to be constant)
P2 = new pressure (to be found)
V2 = new volume (given as 20.0L)
T2 = same as T1 (since the temperature is constant)
Given:
P1 = 1.75 atm
V1 = 10.7 L
V2 = 20.0 L
Substituting these values into the equation:
(1.75 atm * 10.7 L) / T1 = (P2 * 20.0 L) / T1
The T1 cancels out on both sides of the equation, leaving:
1.75 atm * 10.7 L = P2 * 20.0 L
To solve for P2, divide both sides of the equation by 20.0 L:
(1.75 atm * 10.7 L) / 20.0 L = P2
Thus, the new gas pressure (P2) is calculated to be approximately 0.93625 atm.