a flask containing 155cm^3 of hydrogen was collected under a pressure of 22.5 kPa. what pressure would have been required for the volume of gas to have been 90.0 cm^3 assuming the same temperature?

i got 38.75

P1V1= P2V2

is that right?

To solve this problem, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional, assuming constant temperature. Boyle's Law equation is written as:

P1 * V1 = P2 * V2

Where:
P1 = initial pressure (22.5 kPa)
V1 = initial volume (155 cm^3)
P2 = final pressure (unknown)
V2 = final volume (90.0 cm^3)

We can rearrange the equation to solve for P2:

P2 = (P1 * V1) / V2

Now we can substitute the known values into the equation:

P2 = (22.5 kPa * 155 cm^3) / 90.0 cm^3

To simplify the units, we must convert cm^3 to liters and kPa to atm:

1 cm^3 = 1 mL
1 L = 1000 mL
1 kPa = 0.00987 atm

P2 = (22.5 kPa * 155 cm^3) / 90.0 cm^3
P2 = (22.5 kPa * 155 mL) / 90.0 mL
P2 = (22.5 kPa * 155 mL) / (90.0 mL * 1000 mL/L)
P2 = (22.5 kPa * 155 mL * 1 L/1000 mL) / (90.0 mL)
P2 = (22.5 kPa * 155 L) / 90.0
P2 = (0.00987 atm * 155 L) / 90.0
P2 ≈ 0.0169 atm

Therefore, the pressure required for the volume of gas to be 90.0 cm^3, assuming the same temperature, is approximately 0.0169 atm.