Answer :

Final answer:

To find the mass of NO₂ in the tank, we use the Ideal Gas Law, converting the temperature to Kelvin, using the appropriate gas constant, calculating the number of moles, and finally multiplying by the molar mass of NO₂ to get the mass in grams.

Explanation:

The question is asking us to calculate the mass of nitrogen dioxide (NO₂) contained in a 13.0 L tank at a specific temperature and pressure. We can use the Ideal Gas Law for this calculation, which is PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

First, we convert the temperature from Celsius to Kelvin by adding 273.15. So, 112°C is 112 + 273.15 = 385.15 K.

Next, we need to use the ideal gas constant in units consistent with the given pressure (atmospheres) and volume (liters), which is R = 0.0821 L·atm·K⁻¹·mol⁻¹. Then, we rearrange the Ideal Gas Law to solve for n (number of moles) as n = PV / RT.

Plugging the values in, we get n = (4.58 atm) × (13.0 L) / (0.0821 L·atm·K⁻¹·mol⁻¹ × 385.15 K), and solving for n gives us the number of moles of NO₂.

Finally, to find the mass of NO₂, we multiply the number of moles by the molar mass of NO₂, which is 46.0055 g/mol. This will give us the mass in grams of the contents of the tank.

Based on the available options, we would do the calculations and choose the closest answer.

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Rewritten by : Barada