What pressure must be applied to N₂(g) to obtain a density of 2.00 g/L at 25°C?

Question

Quizplus · Accepted Answer

The ideal gas law can be used to calculate the pressure of a gas given its density, temperature, and molar mass. The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. The density of a gas is given by the mass of the gas divided by the volume of the gas. The molar mass of a gas is the mass of one mole of the gas. In this problem, we are given the density of N2(g) and the temperature. We can use the ideal gas law to calculate the pressure of N2(g).First, we need to convert the density of N2(g) from g/L to g/mol. The molar mass of N2(g) is 28.01 g/mol. Therefore, the density of N2(g) is 2.00 g/L * (1 mol/28.01 g) = 0.0714 mol/L.Now, we can use the ideal gas law to calculate the pressure of N2(g). We have:PV = nRTP = nRT/VP = (0.0714 mol/L) * (0.0821 L*atm/(mol*K)) * (298 K) / (1 L)P = 1.75 atmTherefore, the pressure that must be applied to N2(g) to obtain a density of 2.00 g/L at 25°C is 1.75 atm.

What Pressure Must Be Applied to N2(g) to Obtain a Density

What Pressure Must Be Applied to N₂(g) to Obtain a Density