Question

What is the pressure of 1.64 g of nitrogen gas confined to a volume of \(0.170 \ \text{L}\) at \(43^\circ \text{C}\)?

A. Convert the mass of nitrogen to moles.
B. Apply the ideal gas law to find the pressure.
C. Use the given volume and temperature in the calculation.
D. Consider units and round the result to the appropriate precision.

Answer 1

To find the pressure of 1.64 g of nitrogen gas at 43°C in a 0.170 L volume, first convert the mass to moles (0.0585 mol), then apply the ideal gas law with the converted temperature in Kelvin (316 K) to calculate the pressure (≈ 1.77 atm).

Step-by-step explanation:

To calculate the pressure of 1.64 g of nitrogen gas confined to a volume of 0.170 L at 43°C:

1. Convert the mass of nitrogen to moles using the molar mass of molecular nitrogen (N₂), which is 28.01 g/mol.
2. Apply the ideal gas law: PV = nRT, where P is the pressure, V is the volume in liters, n is the number of moles, R is the gas constant (0.0821 L.atm.mol⁻¹.K⁻¹), and T is the temperature in Kelvin.
3. Convert the temperature from Celsius to Kelvin: T = 43 + 273 = 316 K.
4. Substitute the values into the ideal gas law to calculate the pressure.
5. Calculate and round to appropriate precision: