a gas occupies a volume of 5L at a temp. of 20C and a pressure of 1atm. what volume would it occupy at a temp. of 30C and a pressure of 1.1 atm.

(P1V1/T1) = (P2V2/T2)

T must be in kelvin.

To find the volume of the gas at the new conditions, we can use the combined gas law equation, which relates the initial and final states of the gas.

The combined gas law equation is:
(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, respectively.

First, let's convert the temperatures from Celsius to Kelvin. The Kelvin temperature scale is obtained by adding 273.15 to the Celsius temperature.

T1 = 20°C + 273.15 = 293.15 K
T2 = 30°C + 273.15 = 303.15 K

Now we can plug the given values into the combined gas law equation:

(1 atm × 5 L) / (293.15 K) = (1.1 atm × V2) / (303.15 K)

To find V2, we can rearrange the equation:

V2 = (1 atm × 5 L × 303.15 K) / (1.1 atm × 293.15 K)
V2 ≈ 4.99 L

Therefore, the volume of the gas at a temperature of 30°C and a pressure of 1.1 atm would be approximately 4.99 L.