Question

a mixture of gases consists of 26 percent hydrogen, 36 percent helium, and 38 percent nitrogen by volume. calculate the mass fractions of the individual components of the mixture and apparent molecular weight of this mixture. use the table containing the molar mass, gas constant, and critical-point properties.

Answer 1

To calculate the mass fractions of the individual components of the mixture, you need to find the molar masses of hydrogen, helium, and nitrogen. Then, calculate the mass of each component using the percent composition and the total volume of the mixture. Finally, calculate the mass fraction of each component by dividing the mass of each component by the total mass of the mixture.

Step-by-step explanation:

To calculate the mass fractions of the individual components of the mixture, we first need to find the molar masses of hydrogen, helium, and nitrogen. The molar mass of hydrogen (H₂) is 2 g/mol, helium (He) is 4 g/mol, and nitrogen (N₂) is 28 g/mol.

Next, we can calculate the mass of each component using the percent composition and the given total volume of the mixture. For example, if the total volume of the mixture is 100 mL, then there would be 26 mL of hydrogen, 36 mL of helium, and 38 mL of nitrogen.

Finally, we can calculate the mass fraction of each component by dividing the mass of each component by the total mass of the mixture. For example, if the total mass of the mixture is 100 g, then the mass fraction of hydrogen would be (2g / 100g) * 100% = 2%.

Answer 2

To determine the mass fractions for a gas mixture, calculate the moles of each component using their volumes and molar masses, then divide the mass of each component by the total mass. The apparent molecular weight is the sum of each gas's mass fraction times its molar mass.

Step-by-step explanation:

To calculate the mass fractions of individual components of a gas mixture consisting of 26 percent hydrogen (H2), 36 percent helium (He), and 38 percent nitrogen (N2) by volume, we first need to know the molar mass of each gas. From the provided information, molar masses are 2.02 g/mol for H2, 4.00 g/mol for He, and 28.0 g/mol for N2. Let's assume we have 100 liters of the gas mixture. Therefore, it contains 26 liters of H2, 36 liters of He, and 38 liters of N2.

Using the ideal gas law at standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters. Thus, the moles of each gas in the mixture are calculated by the volume of the gas divided by 22.4 liters/mol. Then, the mass of each gas can be calculated by multiplying its moles by its molar mass.

Once the mass of each component is found, the mass fraction of each gas is calculated by dividing the mass of the gas by the total mass of the mixture. To find the apparent molecular weight of the mixture, it is the sum of the products of each component's mass fraction and its molar mass.