What is the identity of a gas that has a density of 1.4975 g/L and a volume of 8.64 L at a pressure of 2.384 atm and with a temperature of 349.6 Kelvin

Answer: H2O (water)

Explanation:

The answer choices for this question are:

A) H2O

B) N2

C) SO2

D) NO3

E) Cl2

The solution of the problem is:

1) dа ta:

density, d = 1.4975 g/liter

volume, V = 8.64 liter

pressure, p = 2.384 atm

temperature, T = 349.6 K

2) Formulas:

d = m/V = > m = d*V

n = m / molar mass = > molar mass = m / n

pV = nRT = > n = pV / RT

3) Solution

n = pV / RT = 2.384 atm * 8.64 liter / (0.0821 atm*liter/K*mol * 349.6K)

n = 0.7176 moles

m = dV = 1.4975 g / liter * 8.64 liter = 12.9384 g

molar mass = m / n = 12.9384 g / 0.7176 moles = 18.03 g/mol

That molar mass corresponds to the molar mass of water, therefore the gas is H2O (water vapor).