Calculate the number of moles in 45.0 g of N₂, and the pressure that it would exert at 20.0°C in a 5.00 L steel tank. A)1.61 mol, 0.525 atm B)1.61 mol, 7.74 atm C)3.21 mol, 15.48 atm D)3.21 mol, 1.05 atm E)6.43 mol, 31.0 atm

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First, calculate the molar mass of N₂ (NIBr). The molar mass is approximately 97 g/mol (N = 14, I = 127, Br = 80). Thus, 45.0 g corresponds to 45.0 g / 97 g/mol = 0.464 mol. Using the ideal gas law PV = nRT, where P is pressure, V is volume (5.00 L), n is the number of moles (0.464 mol), R is the ideal gas constant (0.0821 L·atm/(mol·K)), and T is temperature in Kelvin (20.0°C = 293 K), we can solve for P. P = (nRT)/V = (0.464 mol * 0.0821 L·atm/(mol·K) * 293 K) / 5.00 L ≈ 2.31 atm. However, none of the options exactly match this calculation, suggesting a mistake in the interpretation of the chemical formula or the calculation process. Given the options, B) 1.61 mol, 7.74 atm seems to be the closest to a reasonable outcome if considering potential errors in interpreting the chemical formula or calculation steps. The correct calculation should involve accurately determining the molar mass based on the chemical formula provided and applying the ideal gas law correctly with the given conditions.

Calculate the Number of Moles in 45