A sample of Ammonia gas at 650mmHg and 15 degree has a mass of 56.8g. calculate the volume occupied by the gas. Take N=14, H=1,R=8.3145jk.

The first thing we have to do is change and state all the units so that we can use our ideal gas law equation ().

650 mmHg is a pressure unit, we have to convert this to kiloPascals. We know that 760 mmHg gives us 101 kPa.

P = 86kPa

T = 15°C + 273K = 288K

R (Gas constant) = 8.31 kj/mol  

Molar mass of Ammonia () = (1 x 3) + (14) = 17g/mol

n (moles) = 3.34 mol

V = ?

Rearrange the equation to solve for Volume:

Substitute the values inside:

V =

Therefore 93 L of volume is occupied by the ammonia gas.

there all right good

explanation:

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.