What is the volume of a gas that exerts a pressure of 457 mm Hg, if it excerted a pressure of 250 atm when its volume was 25.0 ml.
Again use P1V1=P2V2, but you will have to convert units.
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To find the volume of the gas when it exerts a pressure of 457 mm Hg, we can use the relationship between pressure and volume known as Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional when temperature is held constant.
We are given the initial pressure P1 = 250 atm and initial volume V1 = 25.0 ml, and we need to find the final volume V2 when the pressure is 457 mm Hg.
First, let's convert the pressure from mm Hg to atm:
1 atm = 760 mm Hg
457 mm Hg * (1 atm / 760 mm Hg) = 0.600 atm
Now we have the initial and final pressures:
P1 = 250 atm
P2 = 0.600 atm
According to Boyle's Law, the product of the initial pressure and volume is equal to the product of the final pressure and volume:
P1 * V1 = P2 * V2
Substituting the known values:
250 atm * 25.0 ml = 0.600 atm * V2
After rearranging the equation to solve for V2, we have:
V2 = (250 atm * 25.0 ml) / 0.600 atm
Calculating this expression:
V2 = 10416.67 ml
Therefore, the volume of the gas when it exerts a pressure of 457 mm Hg is approximately 10416.67 ml.