10.7L of a gas at 1.75 atm are expanded to 20.0L at a mass constant temperature.what the new gas pressure?
Assuming the gas is ideal, we can use Boyle's law:
P1 * V1 = P2 * V2
where
P1 = initial pressure
P2 = final pressure
V1 = initial volume
V2 = final volume
Substituting,
(1.75 atm)(10.7 L) = P2 * 20 L
P2 = 1.75 * 10.7 / 20
P2 = 0.936 atm
Hope this helps~ :3
To find the new gas pressure, we can use Boyle's Law, which states that the product of the initial volume and initial pressure is equal to the product of the final volume and final pressure.
Boyle's Law equation: P₁V₁ = P₂V₂
Given:
Initial volume (V₁) = 10.7 L
Initial pressure (P₁) = 1.75 atm
Final volume (V₂) = 20.0 L
Let's substitute these values into the equation and solve for the final pressure (P₂):
P₁V₁ = P₂V₂
1.75 atm * 10.7 L = P₂ * 20.0 L
Simplifying the equation:
18.725 = P₂ * 20.0
Divide both sides by 20.0 to solve for P₂:
P₂ = 18.725 / 20.0
P₂ ≈ 0.93625 atm
Therefore, the new gas pressure is approximately 0.93625 atm.
To find the new gas pressure, we can use the combined gas law equation, which relates the initial and final states of a gas:
(P1 × V1) / T1 = (P2 × V2) / T2
where
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure (to be found)
V2 = final volume
T2 = final temperature (since the temperature remains constant, T1 and T2 are equal)
Given:
P1 = 1.75 atm
V1 = 10.7 L
V2 = 20.0 L
Substituting the given values into the equation:
(1.75 atm × 10.7 L) / T1 = (P2 × 20.0 L) / T1
We can cancel out the T1 on both sides:
1.75 atm × 10.7 L = P2 × 20.0 L
Now, let's solve for P2:
P2 = (1.75 atm × 10.7 L) / 20.0 L
P2 ≈ 0.93425 atm
Therefore, the new gas pressure is approximately 0.93425 atm.