Final answer:
The pressure inside the tennis ball containing 0.33 g of N2 gas at 24°C is calculated using the Ideal Gas Law and is found to be 2.13 atm, which does not match the provided options. It is recommended to recheck the question for any mistakes.
Step-by-step explanation:
To determine the pressure inside the tennis ball filled with N2 gas, we can use the Ideal Gas Law, which is PV = nRT. Here, P is the pressure we need to find, V is the volume of the ball, n is the number of moles of nitrogen, R is the ideal gas constant, and T is the temperature in Kelvin. First, we convert the mass of N2 to moles: 0.33 g N2 * (1 mol / 28.0 g) = 0.0118 mol Next, convert the temperature to Kelvin: 24°C + 273.15 = 297.15 K And convert the volume to liters: 144 cm³ * (1 L / 1000 cm³) = 0.144 L Now we can solve for P using the ideal gas constant R = 0.0821 L·atm/mol·K: P = nRT / V P = (0.0118 mol)(0.0821 L·atm/mol·K)(297.15 K) / 0.144 L P = 2.13 atm As the answer is not one of the provided options, please double-check for any typos or errors in the question as provided.