Question

What is the density (in g/L ) of hydrogen gas at 24 ∘C and a
pressure of 1640 psi?

Answer 1

The density of hydrogen gas at 24°C and a pressure of 1640 psi is approximately 0.146 g/L.

Step-by-step explanation:

To calculate the density of hydrogen gas at a given temperature and pressure, we can use the ideal gas law equation:

Density (g/L) = (pressure (atm) * molar mass (g/mol)) / (gas constant (L*atm/mol*K) * temperature (K))

First, we need to convert the pressure from psi to atm and the temperature from °C to K. Using the conversion factors, the pressure is equal to 107.27 atm and the temperature is equal to 297.15 K.

Next, we need to determine the molar mass of hydrogen gas. The molar mass of hydrogen is 2 g/mol. Substituting all the values into the equation, we get:

Density = (107.27 atm * 2 g/mol) / (0.0821 L*atm/mol*K * 297.15 K) = 0.146 g/L

Therefore, the density of hydrogen gas at 24°C and a pressure of 1640 psi is approximately 0.146 g/L.

Answer 2

The density of hydrogen gas at 24°C and a pressure of 1640 psi is 1.65 g/L.

Step-by-step explanation:

The density of a gas can be calculated using the ideal gas law. The formula for density is density = (molar mass) x (pressure) / (gas constant) x (temperature).

In this case, we have the temperature in degrees Celsius, so we need to convert it to Kelvin by adding 273.15 (24°C + 273.15 = 297.15K).

The molar mass of hydrogen gas is 2 g/mol, the pressure is 1640 psi, and the gas constant is 0.0821 L atm/mol K.

Calculating the density: density = (2 g/mol) x (1640 psi) / (0.0821 L atm/mol K) x (297.15 K) = 1.65 g/L.