What is the density of carbon dioxide gas (g/L)at 1106.2 mm Hg and 56.3 °C?

Question

Quizplus · Accepted Answer

To solve for density, we can use the ideal gas law: PV = nRT. Rearranging for density gives us: d = (PM)/(RT), where P is the pressure, M is the molar mass, R is the gas constant, and T is the temperature in kelvin. First, we need to convert the pressure from mm Hg to atm: 1106.2 mm Hg = 1.449 atm. Next, we need to determine the molar mass of carbon dioxide, which is approximately 44 g/mol. The gas constant R = 0.0821 L*atm/mol*K. Finally, we need to convert the temperature from degrees Celsius to kelvin: 56.3 °C + 273.15 = 329.45 K. Substituting into the formula: d = (1.449 atm)(44 g/mol)/(0.0821 L*atm/mol*K * 329.45 K) = 2.37 g/L. Therefore, the answer is C.

What Is the Density of Carbon Dioxide Gas (G/L)at 1106