To answer this item, we assume that the gases are ideal for us to be able to use the ideal gas law.
PV = nRT
where P is pressure, V is volume, n is the number of moles, R is the universal gas constant and T is the temperature (in K)
Substituting the known values,
(0.963 atm)(6.92 L) = n(0.0821 L.atm/mol.K)(298 K)
The value of n from the equation is n = 0.27237 moles
We let x and y be the number of moles of NO2 and N2O4, respectively. Given the calculated total moles above and the total mass,
x + y = 0.27237
30x + 60y = 12.55
The values of x and y are:
x = 0.126 moles
y = 0.146 moles
The mole fractions of each gases are therefore:
mole fraction of NO2 = 0.126/(0.126 + 0.146) = 0.46
mole fraction of N2O4 = 0.146/(0.126 + 0.146) = 0.54
Explanation:
colligative properties are properties that depend on the concentration of molecules or ions of the solute, but not on the identity of the solute. Colligative properties include lowering of vapour pressure, boiling point elevation, depression of the freezing point, and osmotic pressure
1) We know that rtp = number of moles × 24
= 0.25 × 24
= 6 dm³
Therefore the volume of 0.25 moles of gas at rtp is A) 6 dm³
3.1) Amount of Copper = 20 tonnes
Amount of pure copper from impure copper = 18 tonnes
Purity of copper = (Pure copper/ impure copper) × 100
= (18 / 20) × 100
= 18 × 5
= 90 %
Therefore the purity of copper is 90%
3.2) We know that oxygen has 8 protons and 8 neutrons, so the weight of oxygen molecule is 8 + 8 = 16 u
So, one mole of oxygen weighs 16 g, so 2 moles weigh 2 × 16 = 32 grams
But oxygen is diatomic so the weight is 32 × 2 = 64 grams
Therefore the weight of 2 moles of oxygen is 64 grams
3.3) Concentration of solution = Amount of solute/volume
= 4 moles/ 2 dm³
= 4 / 2
= 2 mol/dm³
Therefore the concentration of a solution containing 4 moles in 2 dm³ of solution is 2 mol/dm³
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If it is an ionic bond (metal with nonmetal) the electrons will be transferred. If it is a covalent bond (nonmetal with nonmetal) the electrons will be shared. It depends on the electronegativities; the closer the electronegativities of the two atoms, the more covalent the bond is, making the electrons more equally shared. But if the electronegativities are very different, one atom (the nonmetal) will pull the electrons from the other (the metal).
The balanced equation for the above neutralisation reaction is as follows;
2KOH + H₂SO₄ --> K₂SO₄ + 2H₂O
stoichiometry of KOH to H₂SO₄ is 2:1
neutralisation is the reaction between H⁺ ions and OH⁻ ions to form water which is neutral
number of KOH moles - 1.56 mol
2 mol of KOH require 1 mol of H₂SO₄ for neutralisation
therefore 1.56 mol of KOH require - 1/2 x 1.56 mol = 0.78 mol
0.78 mol of H₂SO₄ are required for neutralisation