A gas has a volume of 5.60 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?

To find the final temperature required to cause a change in volume, we can use the combined gas law formula:

(P1 × V1) / (T1) = (P2 × V2) / (T2)

Where:
P1 = initial pressure
V1 = initial volume
T1 = initial temperature
P2 = final pressure
V2 = final volume
T2 = final temperature

In this case, we are given:
V1 = 5.60 L
T1 = 0 °C
V2 = the desired final volume (which is not specified)
P1, P2, and the number of moles of gas (n) are not given, but they are stated as being constant, suggesting that they do not change.

Given that the initial and final pressures are constant, we can simplify the equation to:

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

Substituting the given values:

(5.60 L) / (0 °C) = (V2) / (T2)

To isolate T2, we can cross multiply:

(5.60 L × T2) = (0 °C × V2)

Now, divide both sides by 5.60 L:

T2 = (0 °C × V2) / (5.60 L)

Therefore, to find the final temperature (T2) in degrees Celsius, you need to know the final volume (V2) of the gas. Substitute the desired final volume into the equation, and then solve for T2.