a sample of oxygen that occupies 1.00 x 10^6mL at 575mmHg is subjected to a pressure of 1025atm. what will the final volume of the sample be if the temperature is held constant?

P1V1 = P2V2

just one question how do you find the constant k???

There may be as many as 1000 constants ( or more). Which k do you want?

for combined gas law

Actually, it is never necessary to calculate k. If

(P1V1/T1) = k and
(P2V2/T2) = k, then
(P1V1/T1) = (P2V2/T2)

To answer your question, however, you calculate k from (P1V1/T1) = k

To solve this problem, you can use Boyle's law, which states that the pressure and volume of a gas are inversely proportional when the temperature is constant. Boyle's law is mathematically represented as P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

In this case, we are given:
P1 = 575 mmHg
V1 = 1.00 x 10^6 mL
P2 = 1025 atm
We need to find V2, the final volume.

First, we need to convert the units of pressure and volume to the same system. Since the given pressure is in mmHg and the desired pressure is in atm, we need to convert mmHg to atm. The conversion factor is 1 atm = 760 mmHg. So, P1 becomes 575 mmHg / 760 mmHg/atm = 0.757 atm.

Next, we can plug these values into Boyle's law equation:

0.757 atm * 1.00 x 10^6 mL = 1025 atm * V2

To isolate V2, we divide both sides of the equation by 1025 atm:

V2 = (0.757 atm * 1.00 x 10^6 mL) / 1025 atm

Now we can calculate V2.

V2 = 738,536 mL

Therefore, the final volume of the oxygen sample will be 738,536 mL if the temperature is held constant.