Which of the following statements do you think is the correct one? C. collisions of gas molecules are elastic. Which statement is false? A. The density of a gas is constant as long as its temperature

Here are the solutions to the questions: 9. Which of the following statements do you think is the correct one? C. collisions of gas molecules are elastic According to the Kinetic Molecular Theory of Gases*, collisions between gas molecules are considered perfectly elastic, meaning no net loss of kinetic energy during the collision. 10. Which statement is false? A. The density of a gas is constant as long as its temperature remains constant. The density of a gas depends on both temperature and pressure. Even if the temperature remains constant, a change in pressure will alter the density of the gas. For example, increasing pressure at constant temperature will increase density. 11. A sample of oxygen occupies 47.2 L under a pressure of 1240 torr at 25°C. What volume would it occupy if the pressure were decreased to 730 torr? This problem involves Boyle's Law, which states that for a fixed amount of gas at constant temperature, the pressure and volume are inversely proportional (P_1V_1 = P_2V_2). Step 1: Identify the given values. P_1 = 1240 torr V_1 = 47.2 L P_2 = 730 torr V_2 = ? Step 2: Apply Boyle's Law. P_1V_1 = P_2V_2 Step 3: Solve for V_2. V_2 = (P_1V_1)/(P_2) V_2 = (1240 torr)(47.2 L)730 torr V_2 = 58528 L730 V_2 ≈ 80.175 L Step 4: Choose the closest option. The closest option is D. The volume would be approximately D. 80.2 L. D. 80.2 L 12. A sample of nitrogen occupies 5.50 L under a pressure of 900 torr at 25°C. At what temperature will it occupy 10.0 L at the same pressure? This problem involves Charles's Law, which states that for a fixed amount of gas at constant pressure, the volume and absolute temperature are directly proportional ((V_1)/(T_1) = (V_2)/(T_2)). Step 1: Identify the given values and convert temperature to Kelvin. V_1 = 5.50 L T_1 = 25^ + 273.15 = 298.15 K V_2 = 10.0 L T_2 = ? Step 2: Apply Charles's Law. (V_1)/(T_1) = (V_2)/(T_2) Step 3: Solve for T_2. T_2 = (V_2T_1)/(V_1) T_2 = (10.0 L)(298.15 K)5.50 L T_2 = 2981.5 K5.50 T_2 ≈ 542.09 K Step 4: Convert T_2 back to Celsius. T_2 (in ^) = 542.09 K - 273.15 = 268.94 ^ Step 5: Choose the closest option. The closest option is D. The temperature will be approximately D. 269 °C. D. 269 ^ 13. Under conditions of fixed temperature and amount of gas, Boyle's law requires that D. I, II, and III Boyle's Law states that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional. I. P_1V_1 = P_2V_2: This is a common mathematical expression of Boyle's Law. II. PV = constant: This is the fundamental definition of Boyle's Law. III. P_1/P_2 = V_2/V_1: This is a rearrangement of P_1V_1 = P_2V_2 (P_1V_1 = P_2V_2 P_1/P_2 = V_2/V_1). All three statements correctly represent Boyle's Law. The volume of a sample of nitrogen is 6.00 L at 35°C and 740 torr. What volume will it occupy at STP? This problem involves the Combined Gas Law, which relates pressure, volume, and temperature for a fixed amount of gas ((P_1V_1)/(T_1) = (P_2V_2)/(T_2)). STP (Standard Temperature and Pressure) is 0^ (273.15 K) and 1 atm (760 torr). Step 1: Identify the given values and convert temperatures to Kelvin. V_1 = 6.00 L T_1 = 35^ + 273.15 = 308.15 K P_1 = 740 torr P_2 = 760 torr (STP) T_2 = 0^ + 273.15 = 273.15 K (STP) V_2 = ? Step 2: Apply the Combined Gas Law. (P_1V_1)/(T_1) = (P_2V_2)/(T_2) Step 3: Solve for V_2. V_2 = (P_1V_1T_2)/(P_2T_1) V_2 = (740 torr)(6.00 L)(273.15 K)(760 torr)(308.15 K) V_2 = 1213686 L234194 V_2 ≈ 5.182 L Step 4: Choose the closest option. The closest option is D. (Note: The options provided in the image are A. 6.59 L, B. 5.46 L, C. 6.95 L, D. 5.67 L. My calculated value is not among them. Let me recheck the calculation. V_2 = (740 × 6.00 × 273.15)/(760 × 308.15) = (1213686)/(234194) ≈ 5.182 L. There might be a slight discrepancy with the options or a rounding difference. Let's re-evaluate the options given the calculation. None of the options are close to 5.182 L. Let's re-check the calculation with slightly different rounding or if there's a common mistake. P_1 = 740 torr V_1 = 6.00 L T_1 = 35^ = 308.15 K P_2 = 760 torr T_2 = 0^ = 273.15 K V_2 = V_1 × (P_1)/(P_2) × (T_2)/(T_1) V_2 = 6.00 L × 740 torr760 torr × 273.15 K308.15 K V_2 = 6.00 × 0.97368 × 0.88648 V_2 = 5.84208 × 0.88648 V_2 = 5.182 L The calculation is consistent. Given the options, there might be an error in the question's options or the provided solution (if any was implied by the strike-through on B). If I had to pick the closest, it would be B (5.46 L) or D (5.67 L), but neither is very close to 5.18 L. However, I must provide an answer from the options. Let's assume there's a slight rounding difference or an error in the question's options. I will stick to my calculated value. Since I must choose from the given options, and my calculated value is approximately 5.18 L, none of the options are very close. However, if we consider the possibility of rounding in the options, 5.46 L (B) and 5.67 L (D) are the closest. Let's re-examine the image for any pre-marked answers. Option B has a strike-through, which might indicate it was considered incorrect by a previous attempt. Option D is 5.67 L. Let's re-evaluate the calculation one more time to ensure no arithmetic error. V_2 = (740 × 6.00 × 273.15)/(760 × 308.15) = (1213686)/(234194) ≈ 5.182 L. The calculation is robust. Given the options, there's a significant discrepancy. I will state the calculated value and acknowledge the options. If forced to choose, I would pick the closest, but it's not a good fit. Let's assume there was a typo in the question or options. If the initial volume was slightly different, or the temperature/pressure, it could lead to one of the options. For example, if V_2 was 5.46 L (option B), then P_1V_1/T_1 = P_2V_2/T_2 V_2 = (740 × 6.00 × 273.15)/(760 × 308.15) = 5.182 L. If V_2 was 5.67 L (option D), then V_2 = 5.182 L. Given the discrepancy,