a sample of hydrogen occupies a volume of 950 mL at -15.3 degrees celcius. if the temperature increased to 30.0 degrees celcius, what would be the new volume?

Note the correct spelling of celsius.

Use (V1/T1) = (V2/T2)
T must be in kelvin.

To solve this problem, we can use the ideal gas law equation:

PV = nRT

Where:
P = Pressure (constant)
V = Volume
n = Number of moles (constant)
R = Ideal gas constant
T = Temperature (in Kelvin)

First, let's convert the temperatures from Celsius to Kelvin:

Initial temperature (T1) = -15.3 degrees Celsius
Final temperature (T2) = 30.0 degrees Celsius

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

T1(K) = -15.3 + 273.15 = 257.85 K
T2(K) = 30.0 + 273.15 = 303.15 K

Now, we have the initial volume (V1) = 950 mL = 950 cm³ (since 1 mL = 1 cm³)

Next, we can use the combined gas law equation:

V1 / T1 = V2 / T2

Rearranging the equation for V2, we get:

V2 = (V1 * T2) / T1

Substituting the values we have:

V2 = (950 cm³ * 303.15 K) / 257.85 K

Now, let's calculate the new volume (V2):

V2 = (1.165925 * 10^5 cm³ * K) / K

V2 ≈ 1133.90 cm³

Therefore, the new volume of hydrogen at 30.0 degrees Celsius would be approximately 1133.90 cm³.