Question

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

Answer 1

Answer:

$V=37.05\ L$

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,  

$n=\frac{m}{M}$

Using ideal gas equation as:

$PV=\frac{m}{M}RT$

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:-

$740\times V=\frac{45.0}{30.01}\times 62.36367\times 293.15$

$740V=\frac{822685.94372}{30.01}$

$V=37.05\ L$