POSSIBLE POINTS: 20 1. During a laboratory experiment a student filled a balloon with two different gases, CO_(2) and N_(2) The atmospheric pressure in the laboratory was 103 kPa The partial pressure of the CO_(2) added to the balloon was 40 kPa. What was the partial pressure of the N) in the balloon? 53 kpa 63 kpa 43 kPa 73 kPa

To find the partial pressure of $N_{2}$ in the balloon, we can use Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture.<br /><br />Given information:<br />- Atmospheric pressure in the laboratory: 103 kPa<br />- Partial pressure of $CO_{2}$ added to the balloon: 40 kPa<br /><br />Let's denote the partial pressure of $N_{2}$ in the balloon as $P_{N_{2}}$.<br /><br />According to Dalton's Law of Partial Pressures, the total pressure in the balloon is the sum of the partial pressures of $CO_{2}$ and $N_{2}$:<br /><br />$P_{total} = P_{CO_{2}} + P_{N_{2}}$<br /><br />Substituting the given values:<br /><br />$103 \text{ kPa} = 40 \text{ kPa} + P_{N_{2}}$<br /><br />Solving for $P_{N_{2}}$:<br /><br />$P_{N_{2}} = 103 \text{ kPa} - 40 \text{ kPa} = 63 \text{ kPa}$<br /><br />Therefore, the partial pressure of $N_{2}$ in the balloon is 63 kPa.<br /><br />The correct answer is 63 kPa.