a sample of argon gas at standard pressure ocupies 100ml. at constant temp, what volume does the gas occupy if the temp increases to 800mmHg

You need to get your units straight. T is in kelvin(or celsius), pressure in in mm Hg (or atmosphere or kilopascals).

To find the new volume of the gas when the temperature increases, we need to use the combined gas law equation, which relates the initial and final conditions of pressure, volume, and temperature of a gas sample.

The combined gas law equation is as follows:
(P1 * V1) / T1 = (P2 * V2) / T2

Where:
P1 and P2 are the initial and final pressures of the gas,
V1 and V2 are the initial and final volumes of the gas,
T1 and T2 are the initial and final temperatures of the gas.

In this particular scenario, the pressure and temperature are changing while the volume remains constant, so we can simplify the equation as follows:
(P1 * V1) / T1 = (P2 * V2) / T2

Given that the initial volume (V1) is 100 ml and the initial pressure (P1) is standard pressure (which is approximately 1 atm or 760 mmHg), we can rewrite the equation as:
(760 mmHg * 100 ml) / T1 = (800 mmHg * V2) / T2

Now we can solve for the final volume (V2) by rearranging the equation:
V2 = (760 mmHg * 100 ml * T2) / (T1 * 800 mmHg)

Since the temperature is constant, we can substitute T1 = T2:
V2 = (760 mmHg * 100 ml) / 800 mmHg
V2 = (76000 ml * mmHg) / 800 mmHg
V2 = 95 ml

Therefore, when the temperature increases while keeping the volume constant, the gas will occupy a volume of 95 ml.