Answer:
Explanation:
Given that:
Mass of 
, m = 45.0 g
Molar mass of , 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,
Using ideal gas equation as:
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:-
According to the cooling curve given above, at temperature 275K, the phases that will be observed is LIQUID AND SOLID.
The flat points on the graph represent the points where phase changes are taking place.The beginning of the first flat point represent the point where the gas become liquid, the extreme end of this point indicate the point where the liquid has started turning to liquid and that is the point of 275K. Thus at that point both phases are present.
Since we already have the counts of the number of moles of each element in 1 mole of ammonium nitrate (which are 2 mol N, 4 mol H, 3 mol O), we multiply each of these by the molar masses:
N has a molar mass of 14.0 g/mol, so multiplying by 2 mol N gives 28.0 g N
H has a molar mass of 1.0 g/mol, so multiplying by 4 mol H gives 4.0 g H
O has a molar mass of 16.0 g/mol, so multiplying by 3 mol O gives 48.0 g O
So there are 28.0 g N, 4.0 g H, and 48.0 g O. (The total mass would be 80.0 g ammonium nitrate.)
