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The problem given involves Charles's Law, which states that for a fixed mass of gas at constant pressure, the volume of the gas is directly proportional to its temperature in Kelvin. Mathematically, this is expressed as:

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

Where:
- \( V_1 \) = initial volume = 960 ml
- \( T_1 \) = initial temperature in Kelvin = \( 27^\circ C + 273 = 300 \, K \)
- \( V_2 \) = final volume (unknown)
- \( T_2 \) = final temperature in Kelvin = \( 177^\circ C + 273 = 450 \, K \)

Now, using Charles's Law, we can solve for \( V_2 \):

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

Substituting the values:

\[
V_2 = 960 \, \text{ml} \times \frac{450 \, K}{300 \, K}
\]

Let's calculate the final volume \( V_2 \).The final volume \( V_2 \) that the gas will occupy when the temperature is raised to \( 177^\circ C \) (450 K) is **1440 ml**.

Would you like further details or have any questions? 

Here are five related questions for deeper exploration:
1. What is the general relationship between volume and temperature for an ideal gas?
2. How does Charles's Law differ from Boyle's Law?
3. What happens to the volume if the pressure is not constant but decreases?
4. How would the final volume change if the temperature was decreased instead of increased?
5. What assumptions are made about the gas in Charles's Law?

**Tip:** Always convert temperatures to Kelvin when using gas laws, as Kelvin is the absolute temperature scale used in these equations.

A given mass of gas occupies 960 ml at 27°C. What volume will it occupy if the temperature is raised to 177°C, pressure remaining constant?

Solve the problem of how the volume of a gas changes when the temperature increases from 27°C to 177°C at constant pressure, using Charles's Law. This example covers the application of gas laws, temperature conversion, and proportionality, suitable for high school physics or chemistry.

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