At 25oC temperature and 730 mm pressure, 380 mL of dry oxygen was collected. If the temperature is h — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

# Solution: Gas Law Problem (Constant Temperature) Since temperature is constant and the amount of gas is fixed, apply **Boyle's Law**: $$P_1V_1 = P_2V_2$$ **Given:** - $P_1 = 730$ mm Hg - $V_1 = 380$ mL - $P_2 = 760$ mm Hg - $V_2 = ?$ **Step 1:** Rearrange to solve for $V_2$: $$V_2 = \frac{P_1V_1}{P_2}$$ **Step 2:** Substitute values: $$V_2 = \frac{730 \times 380}{760}$$ **Step 3:** Calculate: $$V_2 = \frac{277,400}{760} = 364.74 \text{ mL} \approx 365 \text{ mL}$$ **Why this is correct:** As pressure increases from 730 to 760 mm Hg, the gas volume decreases proportionally (inverse relationship). The calculated volume of ~365 mL is less than the initial 380 mL, which is physically reasonable.