A sample of gas occupies 3.50 L at 35.0 °C. If the volume is increased to 7.00 L at constant pressure, what is the new temperature of the gas in °C?

• A. 35.0 °C
• B. 70.0 °C
• C. 140 °C
• D. 343 °C

Answer: (D)

Verified step by step guidance

1. Identify the gas law that relates volume and temperature at constant pressure. This is Charles's Law, which states that \(\frac{V_1}{T_1} = \frac{V_2}{T_2}\), where \(V\) is volume and \(T\) is temperature in Kelvin.
2. Convert the initial temperature from Celsius to Kelvin using the formula \(T(K) = T(^\circ C) + 273.15\). So, calculate \(T_1 = 35.0 + 273.15\) K.
3. Write down the known values: initial volume \(V_1 = 3.50\) L, final volume \(V_2 = 7.00\) L, and initial temperature \(T_1\) in Kelvin from the previous step.
4. Rearrange Charles's Law to solve for the final temperature \(T_2\): \(T_2 = \frac{V_2 \times T_1}{V_1}\).
5. Calculate \(T_2\) in Kelvin using the values from step 3 and 4, then convert \(T_2\) back to Celsius by subtracting 273.15: \(T_2(^\circ C) = T_2(K) - 273.15\).