Can anyone help on this chemistry problem, thank you!

Question

A gas has a volume of 3.56 LL at 0 ∘C. What final temperature, in degrees Celsius, is needed to change the volume of the gas to each of the following, if n and P do not change?

for 44.8 mL

Express your answer to three significant figures in degrees Celsius.

Answer 1

Since both P & n are constant you are looking at the direct relationship between volume and (absolute) temperature. That is, in Kelvins. This a an example of Charles' Law: [V ∝T]_{n, P}

So, First change the temp in ^oC to K by adding 273.15. Thus, T₁ = 273.15 K

Next, you are given V₁ in Liters & V₂ in mL. They must be in the same dimensions & it doesn't matter which you choose. For this problem let's make the mL in L: 0.0468 L

Now, we can set up the calculation:

V₁/T₁ = V₂/T₂

Rearrange the equation to solve for T_2: T₂ = (V₂T₁)V₂ = (0.0468 L) (273.15 K)/3.56 L = 3.591 K

They want the answer in ^oC, so we need to subtract the answer in K from 273.15

273.15 K - 3.591 K = 269.6^oC

Correcting to the proper number of sig figs, namely 3, we have 270. ^oC (or 2.70 x 10^{2 o}C)