19. 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_(2) in the balloon? 63 kpa 43 kPa 53 kpa 73 kPa

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19. 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_(2) in the balloon? 63 kpa 43 kPa 53 kpa 73 kPa

Answer 1

Using the formula from step 3, we get: \(P_{N_{2}} = 103 kPa - 40 kPa = 63 kPa\) So, the partial pressure of \(N_{2}\) in the balloon is 63 kPa.

Answer 2

## Step 1: In this problem, we are asked to determine the partial pressure of \(N_{2}\) in the balloon under given atmospheric and \(CO_{2}\) partial pressures. All pressures are given in the same unit (kPa), so no conversion is necessary. ## Step 2: The law of partial pressures, also known as Dalton's law, states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the pressures that each gas would exert alone. Therefore, subtracting the partial pressure of \(CO_{2}\), from the total atmospheric pressure would give us the partial pressure of the \(N_{2}\) gas. ### The formula for Dalton's law is: \(P_{total} = P_{1} + P_{2} + ... + P_{n}\) ## Step 3: Subtract the partial pressure of \(CO_{2}\) from the total atmospheric pressure to find the partial pressure of \(N_{2}\). ### The formula is: \(P_{N_{2}} = P_{total} - P_{CO_{2}}\)

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