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.