This is the chemical formula for acetone: CH32CO. Calculate the mass percent of carbon in acetone.
1 answer:
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Answer:
Explanation:
Hello,
In this case, for the dissociation of calcium fluoride:
The equilibrium expression is:
In such a way, via the ICE procedure, including an initial concentration of calcium of 0.01 M (due to the calcium nitrate solution), the reaction extent is computed as follows:
Thus, the molar solubility equals the reaction extent , therefore:
Regards.
The mentioned molecule with formula, CH₃NO where no bond is found between N and O can be depicted as formamide is shown in the attachment below.
The formal charges = Number of valence electrons for the atom (V) - the number of electrons in lone pairs (N) - 1/2 (number of electrons in bond pairs, B)
FC = V - N - B/2
Thus, there is a need to calculate valence electrons, electrons in lone pairs, and the number of electrons in bond pairs for each atom in the mentioned molecule.
V or valence electrons on C = 4e, on H = 1e, on N = 5e, and on O = 6e.
N or electrons in lone pairs on C = 0e, on H = 0e, on N = 2e, and on O = 4e.
B or number of electrons in bond pairs for C = 8e, for H = 2e, for N = 6e, and for O = 4e.
Thus, the formal charges for each will be,
C = 4 - 0 - (8/2) = 0
H = 1 - 0 - (2/2) = 0
N = 5 - 2 - (6/2) = 0
O = 6 - 4 - (4/2) = 0
Lewis dot structure for the given molecule is given in the attachment below:
Answer:
kp= 3.1 x 10^(-2)
Explanation:
To solve this problem we have to write down the reaction and use the ICE table for pressures:
2SO2 + O2 ⇄ 2SO3
Initial 3.4 atm 1.3 atm 0 atm
Change -2x - x + 2x
Equilibrium 3.4 - 2x 1.3 -x 0.52 atm
In order to know the x value:
2x = 0.52
x=(0.52)/2= 0.26
2SO2 + O2 ⇄ 2SO3
Equilibrium 3.4 - 0.52 1.3 - 0.26 0.52 atm
Equilibrium 2.88 atm 1.04 atm 0.52 atm
with the partial pressure in the equilibrium, we can obtain Kp.