The densities of gases a, b, and c at stp are 1.25 g/l, 2.86 g/l and 0.714 g/l, respectively. calculate the molar mass of each s ubstance. identify each substance as ammonia (nh₃), sulfur dioxide (so₂), chlorine (cl₂), nitrogen (n₂) or methane (ch₄).
1 answer:
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
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Answer:
Explanation:
91.4
grams
Explanation:
C
=
m
o
l
v
o
l
u
m
e
2.45
M
=
m
o
l
0.5
L
2.45
M
⋅
0.5
L
=
m
o
l
m
o
l
=
1.225
Convert no. of moles to grams using the atomic mass of K + Cl
1.225
m
o
l
⋅
(
39.1
+
35.5
)
g
m
o
l
1.225
m
o
l
⋅
74.6
g
m
o
l
=
1.225
⋅
74.6
g
=
91.4
g
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