A sample of helium gas has a volume of 328 mL at 0.69 atm. What pressure is needed to reduce the volume at constant temperature to 32 mL?
Boyles law
P1V1=P2V2
To find the pressure needed to reduce the volume of helium gas, we can use Boyle's Law. Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature. Mathematically, it can be represented as:
P1 * V1 = P2 * V2
where P1 and P2 represent the initial and final pressures, and V1 and V2 represent the initial and final volumes, respectively.
In this case, we have:
P1 = 0.69 atm (initial pressure)
V1 = 328 mL (initial volume)
V2 = 32 mL (final volume)
We need to find P2 (final pressure).
Using the formula, we can rearrange it to solve for P2:
P2 = (P1 * V1) / V2
Substituting the given values:
P2 = (0.69 atm * 328 mL) / 32 mL
Now, let's do the calculation:
P2 = (0.69 atm * 328 mL) / 32 mL
P2 = (226.32 atm * mL) / 32 mL
P2 = 7.07 atm
Therefore, the pressure needed to reduce the volume of the helium gas from 328 mL to 32 mL at a constant temperature is approximately 7.07 atm.