The combustion of carbohydrates and the combustion of fats are both exothermic processes, yet the combustion of carbohydrates is
1 answer:
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Answer:
Equilibrium constant Kc for the reaction will be 1.722
Explanation:
O2(g)+NO(g)→CO(g)+ NO2(g)
0.88 3.9 --- ---
0.88x 3.9-x x x
GIVEN:
0.88X-X= 0.11
⇒ X=0.77
CO2(g)+NO(g) → CO(g) + NO2(g)
0.88 3.9 --- ---
0.88-x 3.9-x x x
= 3.13 0.77 0.77
=0.11
Kc =
=
= 1.722
<u>Answer: </u>The molar mass of the metal is 96.45 g/mol
<u>Explanation:</u>
The fluoride of the metal formed is
The oxidation half-reaction follows:
Calculating the theoretical mass deposited by using Faraday's law, which is:
......(1)
where,
m = actual mass deposited = 1.25 g
M = molar mass of metal = ?
I = average current = 3.86 A
t = time period in seconds = 16.2 min = 972 s (Conversion factor: 1 min = 60 sec)
n = number of electrons exchanged =
F = Faraday's constant = 96500 C
Putting values in equation 1, we get:
Hence, the molar mass of the metal is 96.45 g/mol
Answer:
28.9 g
Explanation:
We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.
<em>Gather all the information in one place</em> with molar masses above the formulas and masses below them.
: 159.69 28.01
Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂
Mass/g: 55.0
1. Use the molar mass of Fe₂O₃ to calculate the moles of Fe₂O₃.
2. Use the molar ratio of CO:Fe₂O₃ to calculate the moles of CO.
3.Use the molar mass of CO to calculate the mass of CO.