The molar mass of a, b and c at STP is calculated as below
At STP T is always= 273 Kelvin and ,P= 1.0 atm
by use of ideal gas equation that is PV =nRT
n(number of moles) = mass/molar mass therefore replace n in the ideal gas equation
that is Pv = (mass/molar mass)RT
multiply both side by molar mass and then divide by Pv to make molar mass the subject of the formula
that is molar mass = (mass x RT)/ PV
density is always = mass/volume
therefore by replacing mass/volume in the equation by density the equation
molar mass=( density xRT)/P where R = 0.082 L.atm/mol.K
the molar mass for a
= (1.25 g/l x0.082 L.atm/mol.k x273k)/1.0atm = 28g/mol
the molar mass of b
=(2.86g/l x0.082L.atm/mol.k x273 k) /1.0 atm = 64 g/mol
the molar mass of c
=0.714g/l x0.082 L.atm/mol.K x273 K) 1.0atm= 16 g/mol
therefore the
gas a is nitrogen N2 since 14 x2= 28 g/mol
gas b =SO2 since 32 +(16x2)= 64g/mol
gas c = methaneCH4 since 12+(1x4) = 16 g/mol
Balanced chemical reaction of hydrochloric acid and barium sulfite:
2HCl(aq) + BaSO₃(s) → BaCl₂(aq) + H₂O(l) + SO₂(g).
Balanced ionic reaction:
2H⁺(aq) + 2Cl⁻(aq) + BaSO₄(s) → Ba²⁺(aq) + 2Cl⁻(aq) + H₂O(l) + SO₂(g).
Net ionic reaction:
2H⁺(aq) + BaSO₄(s) → Ba²⁺(aq) + H₂O(l) + SO₂(g).
Answer:
FIGURE 5.9 The arrow shows a second way of remembering the order in which sublevels fill. Table 5.2 shows the electron configurations of the elements with atomic numbers 1 through 18.
Element Atomic number Electron configuration
sulfur 16 1s22s22p63s23p4
chlorine 17 1s22s22p63s23p5
argon 18 1s22s22p63s23p6
Explanation:
<em>Brainlilest </em><em>me </em>
Answer:
B.Metal B has higher density than metal A
