Question

A sample of gas occupies 4.0 L at 27°C and 1 atm pressure. What will be its volume at 127°C and 1 atm pressure? (Assume ideal gas behavior)

• A. 5.33 L
• B. 60 L
• C. 30 L
• D. 4.33 L

Hint:

Charles's Law is used when pressure is constant: \[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \] Always convert Celsius to Kelvin before applying the gas laws.

Answer 1

The Correct Option is A

Step 1: Use Charles's Law. 
Charles's law: \(\frac{V_1}{T_1} = \frac{V_2}{T_2}\), where temperature is in Kelvin. 
Step 2: Convert Celsius to Kelvin. 
\[ T_1 = 27^\circ C = 300\, K, \quad T_2 = 127^\circ C = 400\, K \] 
Step 3: Apply Charles's Law. 
\[ \frac{V_1}{T_1} = \frac{V_2}{T_2} \Rightarrow \frac{4.0}{300} = \frac{V_2}{400} \Rightarrow V_2 = \frac{4.0 \times 400}{300} = \frac{1600}{300} = 5.\overline{3}\, \text{L} \] 
So, the final volume is approximately 5.33 L.