a 10.0L ballon contains helium gas at a pressure of 655mmHg, what is the new pressure, in mmHg, of the helium gas at 20.0L, if no change in temp or amount of gas
P1V1 =P2V2
To find the new pressure of the helium gas when the volume changes from 10.0 L to 20.0 L, we can use Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional when the temperature and amount of gas are kept constant.
Mathematically, Boyle's Law can be expressed as:
P1 * V1 = P2 * V2
Where:
P1 = initial pressure (in mmHg)
V1 = initial volume (in liters)
P2 = final pressure (in mmHg)
V2 = final volume (in liters)
Plugging in the given values:
P1 = 655 mmHg
V1 = 10.0 L
V2 = 20.0 L
We can rearrange the equation to solve for P2:
P2 = (P1 * V1) / V2
Substituting the values:
P2 = (655 mmHg * 10.0 L) / 20.0 L
P2 = 32775 mmHg / 20.0 L
P2 = 1638.75 mmHg
Therefore, the new pressure of the helium gas at 20.0 L is approximately 1638.75 mmHg.