A sample of krypton gas occupies 95.0 mL at 0.500 atm.

If the temperature remained constant, what volume would
the krypton occupy at (a) 5.00 atm, (b) 0.0500 atm, (c) 555
torr, (d) 5.00 torr, and (e) 5.5 3 1022 torr?

P1V1 = P2V2

To find the volume of krypton gas at different pressures, we can use the ideal gas law equation:

PV = nRT

where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature

In this case, we are assuming the temperature remains constant, so we can rearrange the ideal gas law equation to solve for the volume:

V = (nRT) / P

We are given the initial volume as 95.0 mL and the pressure as 0.500 atm.

(a) To find the volume at 5.00 atm:
Plug the values into the equation: V = (nRT) / P
V = (95.0 mL) * (0.500 atm) / (5.00 atm)
Calculate to find the new volume.

(b) To find the volume at 0.0500 atm:
Again, plug the values into the equation: V = (nRT) / P
V = (95.0 mL) * (0.500 atm) / (0.0500 atm)
Calculate to find the new volume.

(c) To find the volume at 555 torr:
First, convert the pressure to atm: 555 torr / 760 torr/atm = 0.7316 atm
Now, plug the values into the equation: V = (nRT) / P
V = (95.0 mL) * (0.500 atm) / (0.7316 atm)
Calculate to find the new volume.

(d) To find the volume at 5.00 torr:
First, convert the pressure to atm: 5.00 torr / 760 torr/atm = 0.00658 atm
Now, plug the values into the equation: V = (nRT) / P
V = (95.0 mL) * (0.500 atm) / (0.00658 atm)
Calculate to find the new volume.

(e) To find the volume at 5.53 * 10^22 torr:
First, convert the pressure to atm: (5.53 * 10^22 torr) / (760 torr/atm)
Now, convert the result to scientific notation and plug the values into the equation: V = (nRT) / P
V = (95.0 mL) * (0.500 atm) / (converted pressure)
Calculate to find the new volume.

Remember to perform the necessary unit conversions and calculations to find the desired results for each pressure value.