What pressure (in atm) will a sample of o2 gas occupy at 100.0 ml, if o2 has a volume of 25.00 ml at 2.0 atm?

Assuming that the O2 gas acts like an ideal gas, we find the following expression to be approximates of the behaviour of this gas:

P V = n R T                   ---> 1

where,

P = pressure exerted by the gas

V = volume occupied

n = number of moles

R = universal gas constant

T = absolute temperature

Further, we assume that the number of moles and the temperature are constant, hence reducing equation 1 into the form:

P V = k                         ---> 2

where k is a constant. Therefore we can equate two states:

P1 V1 = P2 V2

Since P1, V1 and V2 are given and we are to look for P2:

25 mL * 2 atm = 100 mL * P2

P2 = 0.5 atm

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Explanation:

here's an example: When I was Five i was unconscious after going down a slide into a lake. I was unconscious because on the way down i hit my head on the side. My parents did not know that happened. i was unconscious underwater for a bout a minute until my parents came out to check and see if i was out there because they were looking for me . They did not know where i was. They checked on the boat and found me face down underwater. My dad jumped in to save me and my mom called 911. This was the scariest time in my life and in their life as well. They told me i will never leave their site until i learned not to disobey their rules even if i did not agree with them. I quickly learned to never do things without permission again very fast.