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When fossil fuels are burnt, CO2 is released into the air and is taken up by plants during photosynthesis to form glucose and subsequently starch.
Fossil fuels contain a large proportion of carbon atoms. When fossil fuels are burnt, these carbon atoms are released as carbon dioxide and escape to the atmosphere as atmospheric CO2 in air.
Recall that plants take up the CO2 in air during the process of photosynthesis. This CO2 becomes combined with water in the presence of sunlight to form glucose.
This glucose is converted to starch and stored in plant tissues. This is how the carbon atom inside a fossil fuel becomes a carbon atom inside a plant.
Learn more: brainly.com/question/1388366
Answer:
molecular weight (Mb) = 0.42 g/mol
Explanation:
mass sample (solute) (wb) = 58.125 g
mass sln = 750.0 g = mass solute + mass solvent
∴ solute (b) unknown nonelectrolyte compound
∴ solvent (a): water
⇒ mb = mol solute/Kg solvent (nb/wa)
boiling point:
- ΔT = K*mb = 100.220°C ≅ 373.22 K
∴ K water = 1.86 K.Kg/mol
⇒ Mb = ? (molecular weight) (wb/nb)
⇒ mb = ΔT / K
⇒ mb = (373.22 K) / (1.86 K.Kg/mol)
⇒ mb = 200.656 mol/Kg
∴ mass solvent = 750.0 g - 58.125 g = 691.875 g = 0.692 Kg
moles solute:
⇒ nb = (200.656 mol/Kg)*(0.692 Kg) = 138.83 mol solute
molecular weight:
⇒ Mb = (58.125 g)/(138.83 mol) = 0.42 g/mol
MH₂: 2 g/mol
mO₂: 32 g/mol
2H₂ + O₂ ---> 2H₂O
4g......32g
4g H₂ ---- 32g O₂
Xg H₂ --- 192g O₂
X = (192×4)/32
X = 24g H₂
Answer:
2.56 eV
Explanation:
Using the formula;
ΔE= -RH(1/n^2final - 1/n^2initial)
RH = -2.18 * 10-18 J
nfinal = 2
ninitial =1
Substituting values;
ΔE= -2.18 * 10-18 J(1/4^2 - 1/2^2)
ΔE= -2.18 * 10-18 J(0.0625 - 0.25)
ΔE= 4.09 * 10^-19 J
To convert to eV
4.09 * 10^-19 J/1.6 * 10^-19
=2.56 eV
