What is the density of NO₂ gas at 0.970 atm and 35 ° C?

Question

Quizplus · Accepted Answer

To calculate the density of a gas, we can use the ideal gas law, which states PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin. We can rearrange this equation to solve for density: density = (n * molar mass) / V = (P * molar mass) / (RT). First, we need to calculate the number of moles of gas present. We can use the ideal gas law again, this time solving for n: n = PV / RT. Plugging in the given values and converting Celsius to Kelvin (T = 35 + 273.15 = 308.15 K), we get: n = (0.970 atm) * (1 L) / [(0.0821 L*atm/(mol*K)) * (308.15 K)] = 0.0385 mol. Next, we need to determine the molar mass of NO₂ gas. This can be calculated by adding up the molar masses of each element present, using the periodic table for reference. In this case, we have: N (14.01 g/mol) + O (16.00 g/mol) + S (32.06 g/mol) + 2U (1.01 g/mol) + 2B (10.81 g/mol) = 87.91 g/mol. Finally, we can substitute the values we've calculated into the equation for density: density = (0.970 atm * 87.91 g/mol) / [(0.0821 L*atm/(mol*K)) * (308.15 K)] = 1.76 g/L. Therefore, the best choice is C.

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