Question

What is the volume of 45.0 grams of nitrogen monoxide , NO

at20 degrees celsius and a pressure of 740 mm Hg?

Answer 1

`V=37.05\ L`

Step-by-step explanation:

Given that:

Mass of
`NO`, m = 45.0 g

Molar mass of
`NO`, M = 30.01 g/mol

Temperature = 20.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T₁ = (20.0 + 273.15) K = 293.15 K

V = ?

Pressure = 740 mm Hg

Considering,

`n=(m)/(M)`

Using ideal gas equation as:

`PV=(m)/(M)RT`

where,

P is the pressure

V is the volume

m is the mass of the gas

M is the molar mass of the gas

T is the temperature

R is Gas constant having value = 62.36367 L. mmHg/K. mol

Applying the values in the above equation as:-

`740* V=(45.0)/(30.01)* 62.36367* 293.15`

`740V=(822685.94372)/(30.01)`

`V=37.05\ L`