Question

150°c temperature and 0.987bar pressure and volume will be 0.120dm3. Calculate mass of nitrogen

Answer 1

Explanation:

The given data is as follows.

       P = 0.987 bar = 0.974 atm        (as 1 bar = 0.986 atm)

       T = $150^{o}C$ = (150 + 273) K = 423 K

        V = 0.120 $dm^{3}$ = 0.120 L (as 1 $dm^{3}$ = 1 L)

According to ideal gas equation, PV = nRT

As, n = $\frac{mass}{\text{molar mass}}$

Therefore, putting given values into the above equation as follows.

                   PV = nRT

or,              PV = $\frac{mass}{\text{molar mass}}RT$

            $0.974 atm \times 0.120 L = \frac{mass}{14 g/mol} \times 0.0821 L atm/mol K \times 423 K$

                0.116 = mass × 2.48

                mass = 21.38 g

Thus, we can conclude that mass of nitrogen is 21.38 g.

Answer 2

Answer:The given data is as follows.

P = 0.987 bar = 0.974 atm (as 1 bar = 0.986 atm)

T = = (150 + 273) K = 423 K

V = 0.120 = 0.120 L (as 1 = 1 L)

According to ideal gas equation, PV = nRT

As, n =

Therefore, putting given values into the above equation as follows.

PV = nRT

or, PV =

0.116 = mass × 2.48

mass = 21.38 g

Thus, we can conclude that mass of nitrogen is 21.38 g.

Explanation: