a sample of gas occupies 1910ml at -22.8 degrees C and 740 torr. what volume would it occupy at the same pressure and 285 degrees C? answer units in ml

(P1V1/T1) = (P2V2/T2) but since pressure is the same, you can strike that from the equation.

Remember to convert T to kelvin.

You have to use the combined gas law.

(V1)(P1) / T1 = (V2)(P2) / T2

AND YOU PLUG YOUR GIVEN INTO THE EQUATION.

(1910ML)(740TORR) / -22.8 = (V2)(740TORR) / 285DEGREES

AND SOLVE FOR V2.

To find the volume of the gas at a different temperature but the same pressure, we can use the combined gas law, which is a rearrangement of the ideal gas law. The combined gas law states:

(P1 * V1) / (T1) = (P2 * V2) / (T2)

Where:
P1 and P2 are the initial and final pressures, respectively,
V1 and V2 are the initial and final volumes, respectively,
T1 and T2 are the initial and final temperatures in Kelvin.

Step 1: Convert the initial and final temperatures to Kelvin.
To convert from Celsius to Kelvin, you can use the formula:
T(K) = T(C) + 273.15

Given:
Initial volume (V1) = 1910 mL
Initial temperature (T1) = -22.8 degrees C
Initial pressure (P1) = 740 torr
Final temperature (T2) = 285 degrees C
Final pressure (P2) = 740 torr

Initial temperature in Kelvin:
T1(K) = -22.8 + 273.15 = 250.35 K

Final temperature in Kelvin:
T2(K) = 285 + 273.15 = 558.15 K

Step 2: Rearrange the combined gas law equation to solve for the final volume, V2.
(P1 * V1 * T2) / (T1 * P2) = V2

Plug in the values:
V2 = (P1 * V1 * T2) / (T1 * P2)
= (740 torr * 1910 mL * 558.15 K) / (250.35 K * 740 torr)
= (740 * 1910 * 558.15) / (250.35)
= 29206074 / 250.35
= 116557.06 mL

Therefore, the gas would occupy approximately 116557.06 mL at the same pressure and 285 degrees Celsius.