A sample of gas has a volume of 0.2 lit measured at 1 atm pressure and 0oC. At the same pressure, bu — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

# Solution **Given Information:** - Initial volume: $V_1 = 0.2$ L - Initial temperature: $T_1 = 0°C = 273$ K - Initial pressure: $P_1 = 1$ atm - Final pressure: $P_2 = 1$ atm (same) - Final temperature: $T_2 = 273$ K **Step 1: Identify the gas law to use** Since pressure is constant and we're relating volume to temperature, use **Charles's Law**: $$\frac{V_1}{T_1} = \frac{V_2}{T_2}$$ **Step 2: Substitute values** $$\frac{0.2}{273} = \frac{V_2}{273}$$ **Step 3: Solve for $V_2$** $$V_2 = 0.2 \times \frac{273}{273} = 0.2 \text{ L}$$ **Conclusion:** The volume remains **0.2 L** because the temperature is already at 273 K (which equals 0°C). There is no change in temperature, so by Charles's Law, there is no change in volume at constant pressure. **Answer: B (0.2 L)**