Question

what would the initial volume of a gas has been if it's final volume and temperature are 27L and 370K? Assume the initial temperature was 410K
Charles law

Answer 1

To solve this problem using Charles's Law, we can rearrange the equation as follows:

\[
\frac{V_1}{T_1} = \frac{V_2}{T_2}
\]

where:
- \( V_1 \) is the initial volume,
- \( T_1 \) is the initial temperature (in Kelvin),
- \( V_2 \) is the final volume,
- \( T_2 \) is the final temperature (in Kelvin).

We know the following values:
- \( V_2 = 27 \, L \)
- \( T_2 = 370 \, K \)
- \( T_1 = 410 \, K \)

We can rearrange the equation to solve for \( V_1 \):

\[
V_1 = V_2 \times \frac{T_1}{T_2}
\]

Now, let's plug in the values:

\[
V_1 = 27 \, L \times \frac{410 \, K}{370 \, K}
\]

Calculating that:

\[
V_1 = 27 \, L \times \frac{410}{370}
\]

\[
V_1 = 27 \, L \times 1.1081 \approx 29.93 \, L
\]

Therefore, the initial volume of the gas (\( V_1 \)) would have been approximately **29.93 L**.