Question

What is the density of N₂ gas at 227°C and 5.00 atm pressure?
(R = 0.0821 atm K⁻¹ mol⁻¹) [NEET Kar. 2013]
(a) 0.29 g/ml (b) 1.40 g/ml
(c) 2.81 g/ml (d) 3.41 g/ml

Answer 1

$\huge\underline \mathfrak \blue{Answer}$

(a) 0.29 g/ml

Answer 2

The density of nitrogen gas at given temperature and pressure is 3.41g/ml

Step by step explanation:

According to the ideal gas equation,

                     $\bold{PV = nRT}$.......................(1)

Number of moles can be calculated by the following formula.

           $Number\,of\,moles\,n=\frac{Weight(w)}{Molar\,mass(M)}$

Substitute the "n" value in the equation -1.

                                    $PV= \frac{w}{M(RT)}$

                                           $\Rightarrow PM=\frac{w}{V(RT)}$

                                           $\Rightarrow PM=dRT$

                                           $\bold{\Rightarrow d=\frac{PM}{RT}}$.......................(2)

From the given,

Pressure = P = 5.00 atm

Molar mass = 28 g/mol

Gas constant = 0.0821

Temperature = 227 + 273 = 500 K

Substitute the given values in equation (2)

                                          $\Rightarrow d=\frac{5\times 28}{0.082\times500}$

                                          $\Rightarrow d=3.41g/ml$

Therefore, The density of nitrogen gas at given temperature and pressure is 3.41g/ml

Hence, correct option is "d".

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