a 1.04 l sample of gas at 759 mm hg pressure is expanded until its volume is 2.24 l. what is the pressure in the expanded gas sample at constant temperature
P1*V1=P2*V2
P2=P1*V1/V2=759mmHg(1.04/2.24)
Thanks Bob, that helped me a ton! :)
To solve this problem, we can use Boyle's law, which states that at constant temperature, the product of pressure and volume is constant.
Boyle's Law formula: P1 * V1 = P2 * V2
Given:
P1 = 759 mm Hg
V1 = 1.04 L
V2 = 2.24 L
Let's substitute the values into Boyle's law equation and solve for P2:
P1 * V1 = P2 * V2
759 mm Hg * 1.04 L = P2 * 2.24 L
790.56 = P2 * 2.24
Now, divide both sides by 2.24 to solve for P2:
P2 = 790.56 / 2.24
P2 ≈ 352.71 mm Hg
Therefore, the pressure in the expanded gas sample at constant temperature is approximately 352.71 mm Hg.
To determine the pressure in the expanded gas sample at constant temperature, you can use Boyle's Law. Boyle's Law states that for a fixed amount of gas at constant temperature, the product of its pressure and volume is constant.
Mathematically, Boyle's Law can be represented as:
P1 * V1 = P2 * V2
Where:
P1 = Initial pressure
V1 = Initial volume
P2 = Final pressure
V2 = Final volume
In this case, the initial pressure (P1) is 759 mmHg, the initial volume (V1) is 1.04 L, and the final volume (V2) is 2.24 L.
Substituting the given values into the equation, we can solve for the final pressure (P2):
P1 * V1 = P2 * V2
759 mmHg * 1.04 L = P2 * 2.24 L
790.96 mmHg = P2 * 2.24 L
Now, we can isolate P2 by dividing both sides of the equation by 2.24 L:
P2 = 790.96 mmHg / 2.24 L
P2 ≈ 352.5 mmHg
Therefore, the pressure in the expanded gas sample at constant temperature is approximately 352.5 mmHg.