10.7 L of a gas at 1.75 atm are expanded to 20.0 L at a constant temperature. What is the new gas pressure? *
A canister holds a gas at 16.3 psi when the temperature is 15˚C. To what will the pressure change when the temperature is increased to 20˚C? *
a. P1V1 = P2V2
b. (P1/T1) = (P2/T2)
To find the new gas pressure, we can use Boyle's Law, which states that the product of pressure and volume is constant at a constant temperature.
Boyle's Law equation: P1 * V1 = P2 * V2
Given:
P1 = 1.75 atm (initial pressure)
V1 = 10.7 L (initial volume)
V2 = 20.0 L (final volume)
Let's substitute the given values into the equation and solve for P2 (new pressure).
(1.75 atm) * (10.7 L) = P2 * (20.0 L)
Divide both sides of the equation by 20.0 L to isolate P2:
(1.75 atm * 10.7 L) / 20.0 L = P2
Now let's solve this equation:
(1.75 atm * 10.7 L) / 20.0 L = P2
Multiply 1.75 atm by 10.7 L:
18.725 atm*L / 20.0 L = P2
Divide 18.725 atm*L by 20.0 L:
P2 = 0.93625 atm
Therefore, the new gas pressure is approximately 0.93625 atm.