A gas has a volume of 500 mL at a temperature of -45.0°C. What volume will the gas occupy at 30.0°C? Show your work.

What equation should I use for this one? Sorry but my allergies have me feeling drained. Where should i start on this one?

(V1/T1) = (V2/T2)

Don't forget C must be in kelvin.

Ok, I cross multiplied 500 ml with 303.15 K and I diveded 228.15 K from it.

The result was 664.0 ml. Did I do it in the right order?

To solve this problem, you can use the combined gas law equation:

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

In this equation:
P1 and P2 represent the initial and final pressures of the gas (which are not given in the question).
V1 represents the initial volume of the gas (given as 500 mL).
T1 represents the initial temperature of the gas in Kelvin (you will need to convert -45.0°C to Kelvin).
V2 represents the final volume of the gas (what you are trying to find).
T2 represents the final temperature of the gas in Kelvin (you will need to convert 30.0°C to Kelvin).

Let's start by converting the initial and final temperatures to Kelvin. To convert from Celsius to Kelvin, you use the equation:

Kelvin = Celsius + 273.15

Converting the initial temperature of -45.0°C to Kelvin:

T1 = -45.0 + 273.15 = 228.15 K

Converting the final temperature of 30.0°C to Kelvin:

T2 = 30.0 + 273.15 = 303.15 K

Now that we have the values for V1 (500 mL), T1 (228.15 K), T2 (303.15 K), and we are trying to find V2, we can rewrite the combined gas law equation as:

(V1 * T2) / T1 = V2

Plugging in the values:

(500 mL * 303.15 K) / 228.15 K = V2

Calculating this expression:

V2 ≈ 664.39 mL

Therefore, the gas will occupy approximately 664.39 mL at 30.0°C.