Here's a hint. One of these is a liquid, one is a gas, and one is a radioactive gas. Match each of these descriptions to the right element, and tell me which one you would be most likely to be emitted from your stove.
Answer:
10.49
Explanation:
3MgO + 2Fe — Fe2O3 + 3Mg
n(Fe2O3) = m/M
=15/159.69
=0.9393199324mol
1 Mol of Fe2O3 = 2 moles of Fe
Therefore n(Fe) =2 * 0.9393199324
=0.1878639865mol
m(Fe) = n*m.m
= 0.1878639865 * 55.8
=10.4828g
Answer:
CHO2- ion
Explanation:
We have the lewis structure of a formate-ion here
This is CHO2-.
The carbon atom is the central atom in the structure. It's the least electronegative atom (C). Carbon has 4 valence electrons. Oxygen has 6 valence electrons.
The carbon will bind with 1 hydrogen atom, this will form 1 single bond, because hydrogen has 1 valence electron.
The carbon will bind with oxygen via a double bond.
Since carbon has only 4 valence electrons, it can only form 1 bond with the other oxygen atom.
There will formed 1 double bond between C and O and 1 single bond between C and O resulting in a negative charged O-atom.
This means there are two resonance structures. for the CHO2- ion
The answer is speed
Distance/time=speed
The balanced combustion reaction for one mole of ethane will be
C2H6 + 3.5 O2 ---> 2CO2(g) + 3H2O (l)
Enthalpy of reaction of combustion = ∑ΔHf (products)- ∑ΔHf (reactant)
ΔHf = enthalpy of formation
The enthalpy of formation of oxygen = 0 as it is an element in its native state
ΔHf C2H6 = -83.820 kJ / mole
ΔHf H2O = -285.830 kJ / mole
ΔHf CO2 = -393.509 kJ / mole
ΔHrxn = [2 X ΔHf CO2 + 3 X ΔHf H2O] - [ΔHf C2H6]
ΔHrxn = [2 X (-393.509) + 3 (-285.830)] - [-83.820]
ΔHrxn = -1560.688 kJ / mole
