Question

Under identical conditions of temperature and pressure, which of the following gases has highest density? N₂ 02 NH3 He​

Answer 1

Answer:

correct answer is N2

Explanation:

ρ=PM/RT

N2 M = 28

O2 M = 16

NH3 M = 17

He M = 2

Answer 2

Answer:

The mathematical definition of density is mass divided by volume. The periodic table's elements have different densities, and environmental factors like temperature and atmospheric pressure also have an impact.

Explanation:

We know that density and molar mass can be related as:

                 d = $\frac{PM}{RT}$

where d is the density,

P is the pressure,

M is the molar mass,

T is the temperature.

R is the universal gas constant.

From this expression, we came to know that density is directly proportional to molar mass. As the molar mass increases, the density of that also increases.

The molar mass of N₂ = 2 * 14 g/mol = 28 g/mol

The molar mass of O₂ = 2 * 16 g/mol = 32 g/mol

The molar mass of NH₃ = 1 * 14 g/mol + 3 * 1 g/mol = 17 g/mol

The molar mass of He = 4 g/mol

Hence, O₂ has a higher molar mass among others. So, it possesses the highest density under identical conditions of temperature and pressure.

The correct answer is O₂.

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