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).

Answerit curves up and levels out.explanationwe assume that the container contains absolutely no ammonia to begin with as it states that "nitrogen gas and hydrogen gas" react to "produce ammonia."at dynamic equilibrium, the product and reactant concentrations are equal.this means that, starting from a concentration of zero, [nh₃] must curve "up" from zero and then level out to a constant concentration.