Question

A 2L container will hold about 4g of which of the following gases at 0 degree C and 1 atm? SO_2 N_2 CO_2 C_4H_8 NH_3

Answer 1

None of the listed gases would have a mass of exactly 4g in a 2L container at 0 degrees Celsius and 1 ATM. However, the gas closest to this mass under these conditions would be NH3, with a calculated mass of approximately 1.54g.

Step-by-step explanation:

The question asks which of the following gases: SO2, N2, CO2, C4H8, NH3, would have a mass of approximately 4g if contained in a 2L volume at 0 degrees Celsius and 1 ATM. At standard temperature and pressure (STP), which are conditions of 0 degrees Celsius and 1 atmosphere of pressure, 1 mole of an ideal gas occupies 22.41L. This means that for 2L, we expect approximately 1/11th of a mole of gas. The molecular weights of the gases are as follows: SO2 (64 g/mol), N2 (28 g/mol), CO2 (44 g/mol), C4H8 (56 g/mol), NH3 (17 g/mol). Thus, for each gas, multiplying its molecular weight by 1/11 mole will yield the expected mass of the gas at STP conditions in a 2L container. Only NH3, with a calculation of (17 g/mol)*(1/11 mol) ≈ 1.54 g will be under 4g for the given volume, so none of these gases will have a mass of exactly 4g in a 2L container at these conditions.

Answer 2

To calculate the number of moles and volume in liters of each gas at STP, use the equations moles = mass (g) / molar mass (g/mol) and Liters = moles * 22.41 L/mol.

Step-by-step explanation:

The molar mass of each gas can be used to calculate the number of moles using the equation:

moles = mass (g) / molar mass (g/mol)

Then, we can convert moles to liters at STP using the equation:

Liters = moles * 22.41 L/mol

For example, to calculate the number of moles of CO2:

moles = 4g / 44.01 g/mol = 0.09 mol

Liters = 0.09 mol * 22.41 L/mol = 2.01 L

Using this method, the number of moles and volume in liters of each gas can be calculated.