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

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) Data:

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).

Heat is involved in chemical change in two ways; chemical changes either result in heat being added to or removed from an object, and chemical changes require a certain amount of heat before they can take place.