A gas has a volume of 4.00 at 0. What final temperature in degrees Celsius is needed to cause the volume of the gas to change to the following, if (number of moles of gas) and are not changed?

290 L

(V1/T1) = (V2/T2)

You don't have any units on your numbers. Remember T is in Kelvin.

To find the final temperature in degrees Celsius needed to cause the volume of the gas to change to 290 L, we can use the combined gas law equation.

The combined gas law equation is:

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

where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2, V2, and T2 are the final pressure, volume, and temperature.

In this case, the initial volume is 4.00 L and the final volume is 290 L. We also know that the number of moles of gas (n) and the pressure (P) are not changed.

Assuming constant pressure, the equation can be rearranged to solve for T2:

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

Substituting the given values:

P1 = P2 (since the pressure is not changed)
V1 = 4.00 L
T1 = 0°C (or you can convert it to Kelvin by adding 273.15)
V2 = 290 L

Using the equation, we can calculate the final temperature:

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

T2 = (P1 * 4.00 * 0) / (P2 * 290)

Since (P1 * 4.00 * 0) = 0, the equation simplifies to:

T2 = 0

Therefore, the final temperature needed to cause the volume of the gas to change to 290 L is 0°C.