The question requires that you assume complete ionization of the compound. This is:
(NH4)2 SO4 → 2 NH4 (+) + SO4 (2-)
Then, 1 mol of (NH4)2 SO4 produces 3 moles of ions: 2 moles of NH4 (+) and 1 mol of SO4 (2-)
=> 0.26 * 2 moles of NH4(+) = 0.52 moles of NH4 (+)
0.26 * 1 mol of SO4 (2-) = 0.26 moles of SO4 (2-).
Answer: 0.52 moles of ammonium ions and 0.26 moles of sulfate.ions.
Answer:
2p
Explanation:
To solve this question, we can use Boyle's Law, which states that:
"For a fixed mass of an ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to its volume"
Mathematically:
where
p is the pressure of the gas
V is its volume
The equation can be rewritten as
where in this problem we have:
is the initial pressure of the Xe(g) gas
is the initial volume of the Xe(g) gas
is the final volume of the Xe(g) gas
Solving for p2, we find the final pressure of the gas:
So, the final pressure is twice the initial pressure.
Answer:
10 moles de NO2
Explanation:
Tenemos la ecuación de la reacción como sigue;
N2 (g) + 2 O2 (g) → 2 NO2 (g)
Asi que;
Si 1 mol de nitrógeno produce 2 moles de NO2
5 moles de nitrógeno producirán 5 * 2/1 = 10
Por tanto, se producen 10 moles de NO2 moles
Answer:
548 g/mol
Explanation:
The freezing point depression of a solvent occurs when a nonvolatile solute is added to it. Because of the interactions between solute-solvent, it is more difficult to break the bonds, so the phase change will need more energy, and the freezing point will drop, which is called cryoscopy.
The drop in temperature can be calculated by:
ΔT = Kf*W*i
Where Kf is the cryoscopy constant of the solvent, W is the molality, and i is the van't Hoff factor, which indicates the fraction of the solute that dissolves.
The molality represents how much moles (n) of the solute is presented in each kg of the solvent (m2), thus
W = n/m2
The number of moles is the mass of the solute (m1) in g, divided by the molar mass (M1) of it:
W = m1/(M1*m2)
So, by the data:
0.2214 = 0.632/(M1*0.00521)
0.00115M1 = 0.632
M1 = 548 g/mol
