a sample of carbon dioxide gas occupies 3.5 L at 25degrees C. At what temperature will the gas volume be 1 L?

V1/T1 = V2/T2

Use T in Kelvin.

v2xt1/v1=t2

1x298/3.5=85.1k

If your teacher is picky about significant figures, I think you are allowed only two (from the 3.5) and I assume the 1 L actually is 1.0 L. If so, I would round to 85 K.

To find the temperature at which the gas volume will be 1 L, we can use the combined gas law equation. The combined gas law relates the pressure, volume, and temperature of a gas sample.

The formula for the combined gas law is:

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

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

In the given problem, we know:
V1 = 3.5 L (initial volume)
T1 = 25 degrees C (initial temperature)
V2 = 1 L (final volume)

The next step is to convert the initial and final temperatures to Kelvin since the temperature in the gas law equations should be in Kelvin.

To convert Celsius to Kelvin, we use the formula:
T(K) = T(C) + 273.15

So, converting T1 = 25 degrees C to Kelvin,
T1(K) = 25 + 273.15 = 298.15 K

Now, we can rearrange the combined gas law equation and solve for T2:

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

Since we're assuming constant pressure, we can simplify the equation:

(V1 * T2) = (V2 * T1)

Now, we can substitute the known values:
(3.5 * 298.15) = (1 * T2)

Solving for T2:
T2 = (3.5 * 298.15) / 1
T2 = 1044.03 K

Therefore, the gas volume will be 1 L at a temperature of approximately 1044.03 Kelvin.