Question

A sample of an unknown compound is vaporized at 170°C. The gas produced has a volume of 2280 mL and weighs 2.01 g at a pressure of 1 atm. Based on its molar mass, what is the most likely identity of the unknown gas?

A. N2
B. CO2
C. CO
D. O2
E. F2

Answer 1

Comparing the calculated molar mass to the choices given, we can see that the most likely identity of the unknown gas is option a) N2.To determine the most likely identity of the unknown gas, we can calculate its molar mass based on the given information.

Step-by-step explanation:

To determine the most likely identity of the unknown gas, we can calculate its molar mass based on the given information.

First, we convert the volume from mL to L: 2280 mL / 1000 = 2.280 L.

Next, we use the ideal gas law equation PV = nRT to calculate the number of moles of the gas.

Rearranging the equation, we have n = PV / RT.

Substituting the given values, we get n = (1 atm)(2.280 L) / (0.0821 L·atm/mol·K)(170°C + 273).

Calculating n, we find that it is approximately 0.0911 mol.

Lastly, we can calculate the molar mass of the gas using the formula molar mass = mass / moles. Substituting the given mass of 2.01 g and the calculated moles of 0.0911 mol, we find that the molar mass is approximately 22.07 g/mol.

Comparing the calculated molar mass to the choices given, we can see that the most likely identity of the unknown gas is N2.