To determine the new volume of the gas at standard atmospheric pressure, we need to use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when the temperature is constant.
Boyle's Law equation: P1V1 = P2V2
Where:
P1 = initial pressure = 850 torr
V1 = initial volume = 0.5 L
P2 = final pressure (standard atmospheric pressure) = 1 atm
V2 = final volume (to be determined)
We can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Let's substitute the given values into the equation:
V2 = (850 torr * 0.5 L) / 1 atm
Before calculating, we need to convert torr to atm:
1 atm = 760 torr
V2 = (850/760) * 0.5 L
V2 = 0.559 L
Therefore, the gas would occupy approximately 0.559 L at standard atmospheric pressure.
A sample of gas occupies 0.5L at 850tor what volume does it occupy at standard atomospheric pressure (tempreture is conistant)
1 answer