Answer: D
Explanation:
London forces become stronger as the atom in question becomes larger, and to a smaller degree for large molecules. [4] This is due to the increased polarizability of molecules with larger, more dispersed electron clouds. The polarizability is a measure of ease with which electrons can be redistributed; a large polarizability implies that the electrons are more easily redistributed. This trend is exemplified by the halogens (from smallest to largest: F 2 , Cl2 , Br 2 , I 2 ). The same increase of dispersive attraction occurs within and between organic molecules in the order RF<RCL<RBr<RI, or with other more polarizable heteroatoms. [5] Fluorine and chlorine are
gases at room temperature, bromine is a liquid, and iodine is a solid. The London forces are thought to be arise from the motion of electrons.
Ncomplete combustion of<span> fossil </span>fuels<span>; forest fires// heavy traffic ... NS: </span>oxidation<span> of H2S </span>gas<span>from </span>decay<span> of </span>organic matter<span> & volcanic activity ... primary pollutant; </span>burning<span> of </span>sulfur containing<span>fossil </span>fuels<span>, </span>coal<span> containing ... HS: </span>combustion of<span> fossil </span>fuel<span>, industrial plants that </span>produce<span> smoke, ash, dust ..... </span>photochemical<span> smog.</span>
The higher the energy density of a fuel, the greater the amount of energy it has stored.
<h3>What is the energy density?</h3>
The energy density of a fuel is defined as the amount of energy it possesses per unit volume or per unit weight.
<h3>Characteristics of the energy density</h3>
- It is the amount of energy accumulated in an energy vector per unit volume or mass.
- In general, higher density energy sources and carriers are preferable, as many end uses require concentration of such energy.
- The packaging of energy in liquid hydrocarbons is the one with the highest energy density, that is, the highest energy per volume unit, hence its high use in the transportation sector.
Therefore, we can conclude that in general, fuels, especially low molecular weight fuels, have high energy densities.
Learn more about the energy density here: brainly.com/question/2165966
Answer:
+523 kJ.
Explanation:
The following data will be used to calculate the average C-S bond energy in CS2(l).
S(s) ---> S(g)
ΔH = 223 kJ/mol
C(s) ---> C(g)
ΔH = 715 kJ/mol
Enthalpy of formation of CS2(l)
ΔH = 88 kJ/mol
CS2(l) ---> CS2(g)
ΔH = 27 kJ/mol
CS2(g) --> C(g) + 2S(g)
So we must construct it stepwise.
1: C(s) ---> C(g) ΔH = 715 kJ
2: 2S(s) ---> 2S(g) ΔH = 446 kJ
adding 1 + 2 = 3
ΔH = 715 + 446
= 1161 kJ
3: C(s) + 2S(s) --> C(g) + 2S(g) ΔH = 1161 kJ
4: C(s) + 2S(s) --> CS2(l) ΔH = 88 kJ
adding (reversed 3) from 4 = 5
ΔH = -1161 + 88
= -1073 kJ
5: C(g) + 2S(g) --> CS2(l) ΔH = -1073 kJ
6: CS2(l) ---> CS2(g) ΔH = 27 kJ
adding 5 + 6 = 7
ΔH = -1073 + 27
= -1046 kJ
7. C(g) + 2S(g) --> CS2(g) ΔH = -1046 kJ
Reverse and divide by 2 for C-S bond enthalpy
= -(-1046)/2
= +523 kJ.
